Entropy of hcl gas. 4 g of nitrogen gas is heated at a constant pressure of 1.

Entropy of hcl gas 4 g of nitrogen gas is heated at a constant pressure of 1. Al(g) 330. 2 J mol-1 K-1}$. For an ideal gas mixture or an ideal solution, there is no enthalpy of mixing (), so that the The N 2-HCl gas mixture at varying partial pressure of HCl was bubbled to ChCl-EG (1:2) solvent in the absorption setup (Fig. Reason: 2 moles of gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; French, Ikuta, et al. As the reaction is exothermic, the installation is called an HCl oven or HCl burner. Substituting for the definition of work for a gas. 4 J K − 1 m o l − 1 When you heat up a gas in a closed container, you give the molecules additional energy. Click on the group to access the table for that group. [ Cl^- + H_2SO_4 \rightarrow HCl + HSO_4^- \nonumber \] The full equation for the reaction is: \[ NaCl + H_2SO_4 \rightarrow HCl + NaHSO_4 \nonumber \] For simplicity, entropy can be thought of as a measure of the amount of disorder in a NIST/TRC Web Thermo Tables (WTT) NIST Standard Reference Subscription Database 3 - Professional Edition Version 2-2012-1-Pro This web application provides access to a collection of critically evaluated thermodynamic property data for pure compounds with a primary focus on organics. 25 hPa and temperature 25 °C. −704. 8 L. (ΔH < 0), such as during the With our entropy calculator, you can determine the entropy change of chemical reactions and the isothermal entropy change of ideal gases. 7 J K − 1 m o l − 1 = 373. A table of standard molar entropies at 0K would be pretty useless because it would be 0 for every substance (duh!) The compound hydrogen chloride has the chemical formula HCl and as such is a hydrogen halide. S. 7 J Ki mol-rxn The lowered entropy reflects the greater order of the solution state over the gaseous state. Standard Enthalpies of Formation. J. (c) The HCl sample has the higher entropy because the HCl molecule is capable of storing energy in more ways than is Ar. If we fix the amount to one mole, the 1M HCl would be within 1 liter. [1] When a substance or compound is combined with any other substance or compound, the enthalpy of mixing is the consequence of the new interactions between the two substances or compounds. Place the following in order of decreasing molar entropy at 298 K. 5)+1\ln(0. All rights reserved. Most of data from Ebbing, Darrell D. 964 Cesium Chloride: Solid CsCl -443. AlCl 3 (s). S1) e. It also allows us to predict the final state of a sample of a gas (i. Aluminum: Al(s) 0. The hydrogen halides are colorless gases at room temperature, producing steamy fumes in moist air. Unlike the chemical reaction entropy generation, the gas diffusion entropy generation in a combustor with PBNOS increases gradually as the swirler height decreases. The reaction, 9. These data were generated through dynamic data analysis, as implemented in the The entropy of a substance is influenced by the structure of the particles (atoms or molecules) that comprise the substance. HCl N_2H_4 Ar A: N_2H_4 greater than Ar greater than HCl. ΔG f ° (kJ/mol). Calculate the entropy change for 1. The Gas Constant, R, is equal to 8. 01 96. The ideal gas law allows us to calculate the value of the fourth variable for a gaseous sample if we know the values of any three of the four variables (P, V, T, and n). Standard Molar Entropy, S 0 The entropy of a substance has an absolute value of 0 entropy at 0 K. (The molar specific heats are C_v is 20. ΔH f ° (kJ/mol). 289. The predicted molar enthalpy values show excellent agreements compared to the experimental data in a wide temperature range for the gases CO, HCl, and BF. 0708% and 0. Linstrom and W. its value is positive. 0500 mol of HCl(aq) reacts with 0. 109. To proceed systematically, substitute the explicit formula for Q for a gas of independ-ent, indistinguishable molecules (see eqn 16. Standard entropy of the substance refers to so-called standard conditions i. 0500 mol of NaOH(aq) to form 0. Thermodynamic Data: Calculate the change in entropy (in J/K) when 61. As a result, it has higher molar The observed trend, which was expected, indicated that the stability of the HCL product in gaseous phase increased with T. 0500 mol of NaCl(aq), 2. Three stoppered flasks are shown with right and left-facing arrows in between each; the first is labeled above as, “delta S greater than 0,” and below as, “delta S less than 0,” while the second is labeled above as, “delta S greater Entropy, a brief discussion on entropy change and its effect on the spontaneity of a Process, spontaneity of a reaction, the expression for entropy change and more with Byju's. 4 Effusion and Diffusion of Gases; 9. P. It is the heat content of a system. 4 (C), the results obtained show that increasing the temperature leads to an evident reduction in the standard molar entropy of formation of HCl in the gaseous phase. Readers of this section who have had some exposure to thermodynamics will know that solubility, like all equilibria, is governed by the Enthalpy. Gas Phase Heat Capacity (Shomate Equation) References; Notes; Other data available: Gas phase thermochemistry data; Phase change data; Reaction thermochemistry data: reactions 1 to 50, reactions 51 to 100, reactions 101 to 150, reactions 151 to 158; Henry's Law data; Gas phase ion energetics data; Ion clustering data; IR Spectrum; Mass spectrum Solids, Liquids, and Gases Perhaps the most obvious feature of the table of molecular entropies is a general increase in the molar entropy as we move from solids to liquids to gases. Ideal gas thermodynamic properties: heat capacity, enthalpy, entropy, enthalpy function, Gibbs energy function, enthalpy of formation, and Gibbs energy of formation from 0 to 1500K or 0 to 3000 K; Properties as Functions of Selected Temperatures. Solution. What is ΔH, the enthalpy change, per mole of acid reacting, for the acid-base reaction run The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298. 9 = 118. where. Chemists use the term "entropy" to denote this aspect of molecular randomness. condensation) results in an decrease in the disorder of the substance, and a decrease in the entropy ; A chemical reaction between gas When you heat $\ce{NH4Cl}$ it decomposes into $\ce{NH3 + HCl}$ gases. ΔS°(reaction) = 188. HCl molecules can rotate and vibrate; Ar atoms cannot. Mallard, Eds, NIST Chemistry WebBook, NIST Standard Reference Database ΔH° f: The standard enthalpy of formation at 25°C (298,15 K) for 1 mol of the substance in its given state (g= gas and l= liquide) from its elements in their standard state (stable forms at 1 bar and 25°C) ΔG° f: The standard Gibbs free energy of formation at 25°C (298,15 K) for 1 mol of the substance in its given state (g= gas and l= liquide) from its elements in their standard state The pure chlorine gas can be combined with hydrogen to produce hydrogen chloride in the presence of UV light. The resulting hydrogen chloride gas is The thermodyamic properties are arranged by group from the periodic table. 5 J K•mol (1 mol) - 186. The enthalpy change of solution is the enthalpy change when 1 mole of an ionic substance dissolves in water to give a solution of infinite dilution. g. 1M HCl would be within 10 liters. 3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions; 9. , its final temperature, pressure, volume, and amount) following any changes in conditions if the HCl(gas)=HCl(aqueous) (4) For reaction (3) AH° can be computed from data on the temperature coefficientof the emf of cells, and for reaction (4) itis known from Calculate the standard enthalpy and entropy changes for the formation of HCl(g) from gaseous hydrogen and chlorine. 5 Hydrofluoric Acid: Gas HF -269 Hydrochloric acid: Gas HCl The third law of thermodynamics has two important consequences: it defines the sign of the entropy of any substance at temperatures above absolute zero as positive, and it provides a fixed reference point that allows us Applying the Ideal Gas Law. S° (J/mol K). 2 Standard Heats and Free Energies of Formation and Absolute Entropies of Elements and Inorganic Compounds The entropy of a gas is much greater than that of a liquid because gaseous particles are very far apart from each other and can move freely at great speeds. Flame inside HCl oven. 5 The Kinetic-Molecular The Gibbs energy of a Gas: standard states. 1 Gas Pressure; 9. Secretary of Commerce on behalf of the U. For a given substance, the entropy of the liquid state is greater than the entropy of the solid state. 2 J K•mol (1 mol) = -129. 5))=2R\ln(2)$ where the mole fraction is $0. 0. In the accompanying text of this tool, you'll learn: What entropy is; How to calculate the entropy change of a reaction; The entropy calculator helps to estimate the entropy change of a chemical reaction in seconds. According to Fig. 0. Now the molecules have more ways of spreading energy than before, so increasing temperature increases entropy (you can also use this method to Example \(\PageIndex{1}\): Entropy Change for a Gas Expansion. {HCl}\) (a white, choking gas), in water you get an entirely new chemical substance: hydrochloric acid (or muriatic acid as it is known in hardware stores), one of the The heterolytic bond dissociation energy step is a gas phase Brønsted acid base reaction: \[\ce{HA(g) → H^{+}(g) + A^{-}(g)} \nonumber \] Consequently it will be important to consider gas phase acidity before Enthalpy change of solution. Standand Enthalpies of Formation & Standard Entropies of Common Compounds Substance State ∆H f S (kJmol) (Jmol·K) Ag s 0 42. the 0. In a solid, the molecules are only capable of restricted vibrations around a fixed point, but when a solid melts, the molecules, though still hampered by their mutual attraction, are much S° gas,1 bar: Entropy of gas at standard conditions (1 bar) T c: Critical temperature: T fus: Fusion (melting) point: Δ f H° gas: Enthalpy of formation of gas at standard conditions: Δ sub H: Enthalpy of sublimation: Δ vap H: The quantity \(S\subs{m,0}\) in the last column is the difference between the two \(S\m\st\) values, and is called the molar residual entropy. 4 L to 48. Cl 2 (g) + H 2 (g) → 2 HCl(g) As the reaction is exothermic, the installation is called an HCl oven or HCl burner. [1] This enthalpy, if released We can predict whether a reaction will occur spontaneously by combining the entropy, enthalpy, and temperature of a system in a new state function called Gibbs free energy (G). 0; Options: Switch to calorie-based units; Data at NIST subscription sites: The predicted molar Gibbs free energies are in excellent agreement with the experimental data in a wide temperature range for three gases under consideration, and the average absolute deviations of the predicted results from the experimental data are 0. 164. 7 - 69. 2. 314 J/mol·K. 16696% for the gases Cl 2, Br 2, and HCl, respectively. 4. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. My question is why does it decompose into ammonia and hydrogen chloride gases on the molecular level. Related to this Question. If we think about the particulate space, there are billions more microstates 1 mol of HCl particles can occupy in 10 L of space compared to 1 L of space. We begin by using the first law of thermodynamics: dE = dQ - dW where E is the internal energy and W is the work done by the system. 8. The change in entropy is only due to the fact that the volume of each gas is increased, not the mixing per se. 2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law; 9. The proposed Rigid Rotor Assumption and Rotamers. The predicted molar Gibbs free energies are in excellent agreement with the experimental data in a wide temperature range for three gases under consideration, and the average absolute deviations of the predicted results from the experimental data are 0. 83 Water Gas H 2 O -241. For example, an isothermal reversible expansion of an ideal Increase - the melting of ice cubes at 10∘C and 1 \(\rm atm\) pressure - the dissolution of \(\rm HCl(g)\) in water to form concentrated hydrochloric acid Decrease - alignment of iron filings in a magnetic field - the reaction of sodium metal with chlorine gas to form sodium chloride - separating a mixture of \(\rm N_2\) and \(\rm O_2\) into two separate samples, one that is pure The number of gas molecules increases. The change in free energy, \(\Delta G\), is equal to the sum of the enthalpy plus the product of the temperature and entropy of the system. A table of standard molar entropies at 0K would be pretty useless because it would be 0 for every S° gas,1 bar: Entropy of gas at standard conditions (1 bar) T c: Critical temperature: T fus: Fusion (melting) point: Δ f H° gas: Enthalpy of formation of gas at standard conditions: Δ r G° Free energy of reaction at standard conditions: Δ r H° Enthalpy of reaction at standard conditions: Δ vap H: Enthalpy of vaporization When 0. The more “mixed up” or “disorderly” or “messy” a system becomes, we say the entropy of the system increases. As a result, when the sign of entropy change {eq}\left( {\Delta S} \right) {/eq} is positive, the reaction will happen on its Also learn about entropy specific to gases, examples that use the entropy formula, and applications. The same result is true for any two different inert gases no matter how alike or not they may be. −628. Basing on the the standard entropies of all substrates and Standard Entropies Alan D. 04 Chlorine: Chlorine: Gas Cl 2: 0 Chromium: Copper: Fluorine: Fluorine: Gas F 2: Hydrogen: Hydrogen: Gas H 2: 0 Water Liquid H 2 O -285. 7 J mol-1 K-1}$ so the entropy of neon is expected to be smaller by about $\pu{15. the enthalpy and entropy of gas dissolution, and more importantly to predict the absorption behavior at specified design conditions, which is vital for the optimization and design of an absorption/desorption Similarly, the translational entropy of neon is $\pu{3. 06155%, 0. the entropy of a pure substance at 298 K and 1 atm pressure). . The pressure of a perfect gas does not affect its enthalpy, but it does affect the entropy (box at left), and thus, through the –TΔS term, the free energy. (1) ΔG° = – R T ln K = ΔH° – TΔS° Calculate the change in the standard molar entropy of hydrogen chloride, HCl, gas when it is heated from a temperature of 20°C to 30°C. , General Chemistry, Because the entropy of a substance depends on the amount of substance, the pressure, and the temperature, it is convenient to describe the entropy of a substance in terms Entropy, S, is defined as the measure of the disorder or randomness in a system. 8^oC. 00 mol of an ideal gas expanding isothermally from a volume of 24. 3 at the end of the chapter) into eqn 17. 5$. The entropy increase is $\Delta S=-R(1\ln(0. The standard molar constant-pressure heat capacity of hydrogen chloride is 29. 8 J K-1 mol-1. Therefore, entropy increases in processes in which solid or liquid reactants form gaseous products. You'll also be able to study a process' spontaneity through the Gibbs free energy equation. 7 AgCl s −127. The proposed model is away from the need of plenty of experimental spectroscopy data, and S° gas,1 bar Entropy of gas at standard conditions (1 bar) Δ f H° gas: Enthalpy of formation of gas at standard conditions Gibbs free energy, denoted \(G\), combines enthalpy and entropy into a single value. See more By formula: Cl -+HCl = (Cl -•HCl) Bond type: Hydrogen bond (negative ion to hydride) gas phase; Affinity: shift in apparent EA from lesser-solvated ion. This quantity combines two physical effects—the enthalpy of mixing, which is a measure of the energy change, and the entropy of mixing considered here. The increase in entropy is expected with the transition to the disordered state of a gas. What Is Entropy In Chemistry? “It is a measurable physical property that is most commonly associated with uncertainty” Substance. Entropy of an Ideal Gas. Based on the diagram, which of the following best predicts and explains the sign of the entropy change for the reaction, ΔS°rxn ? A ΔS°rxn is negative because the number of N2O4 molecules increases as We can trace the reason for this back to the entropy of solution. Likewise, the entropy of the gas is greater than the entropy of the liquid. Enthalpy is a central factor in thermodynamics. Hydrogen chloride is produced by combining chlorine and hydrogen: Cl 2 + H 2 → 2 HCl. 78 Hydrogen Cyanide: Gas HCN +130. 28. The entropy S of a monoatomic ideal gas can be expressed in a famous equation called the Sackur-Tetrode equation. A. Sgas >> Sliquid > Ssolid. Answer For a gas of independent molecules, Q =qN/N! with q =V/Λ3: p =kT In thermodynamics, the enthalpy of mixing (also heat of mixing and excess enthalpy) is the enthalpy liberated or absorbed from a substance upon mixing. pressure 1013. 3. Standard molar entropies are listed for a reference temperature (like 298 K) and 1 atm pressure (i. , 1986: gas phase; From thermochemical cycle(Cl-)H2O/HCl, Entropy change calculated or estimated; Keesee and Castleman, 1980; M: Quantity Value Units Method Reference Comment Table A–1 Molar mass, gas constant, and critical-point properties Table A–2 Ideal-gas specific heats of various common gases Table A–3 Properties of common liquids, solids, of formation, and absolute entropy at 25°C, 1 atm Table A–27 Properties of some common fuels and hydrocarbons Table A–28 Natural logarithms of the equilibrium Enthalpy of formation (Hfg), Entropy, Integrated heat capacity (0 K to 298. In general, the entropy change for a reaction can be determined if the standard entropies of each substance Entropy: In thermodynamics, a reaction is said to be spontaneous if its entropy is greater than zero, i. 50 atm from 25. 1 J K –1 mol –1. 45 and Table 17. 6. C: HCl greater than N_2H_4 greater than Ar. Trouton's rule validity S° gas,1 bar: Entropy of gas at standard conditions (1 bar) T c: Critical temperature: T fus: Fusion (melting) point: Δ f H° gas: Enthalpy of formation of gas at standard conditions: Δ r G° Free energy of reaction at standard Entropy change for reaction = Entropy of product - Entropy of reactant. You can also determine the Gibbs free energy and isothermal entropy change of an ideal gas. When the pressure of such a gas changes from \(P_1\) to \(P_2\), the Gibbs energy change is A phase change from a liquid to a solid (i. dQ = dE + p dV where p is the pressure and V is the volume of the gas. Recognizing that this is an isothermal process, we can use Equation \ref{isothermS} Gas phase thermochemistry data; Reaction thermochemistry data; Gas phase ion energetics data; Options: Switch to calorie-based units; Data at NIST subscription sites: NIST / TRC Web Thermo Tables, professional edition (thermophysical and thermochemical data) Entropy of liquid at standard conditions (1 bar) We present a universal efficient closed-form representation for the molar enthalpy of gaseous substances. Go To: Top, References, Notes Data compilation copyrightby the U. 15 K) (HH), Heat Capacity (Cp) Standard Molar Entropy, S 0 The entropy of a substance has an absolute value of 0 entropy at 0 K. 83 Hydrogen Peroxide: Liquid H 2 O 2-187. condensation) results in an decrease in the disorder of the substance, and a decrease in the entropy ; A chemical reaction between gas molecules that Study with Quizlet and memorize flashcards containing terms like The diagram above represents the gas-phase reaction of NO2(g) to form N2O4(g) at a certain temperature. Entropy and Free Energy 307 (d) HCl (g) → HCl (aq) ∆rS˚ = 56. 79 72. At room temperature, it is a colorless gas, which forms white fumes of hydrochloric acid upon contact with atmospheric water So $$\ce{Mg(s) + 2 HCl(aq) -> H2(g) + MgCl2(aq) + Heat}$$ From a conceptual standpoint, shouldn't the change in entropy be positive for this reaction because there are more moles of gas in the Another order of magnitude reduction in the pressure of the gas and the entropy change would be favorable by $ \pu{17. 15 K or 25 °C). N = number of atoms k = Boltzmann's constant V = volume U = internal energy h = Planck's constant One of the things which can be determined directly from this equation is the change in entropy during an isothermal expansion Molar Entropy would be an entropy/mol quantity. Is it because in the $\ce{N-(HCl)}$ The general cases below illustrate entropy at the molecular level. Separation of the rotational partition function from the partition functions of other degrees of freedom does not only require consideration of nuclear spin states, but also the assumption that The Gibbs free energy change = determines whether mixing at constant (absolute) temperature and pressure is a spontaneous process. , 1982; M: Δ r S° 95. Share. B: Ar greater than N_2H_4 greater than HCl. A phase change from a liquid to a solid (i. 8^oC to 92. A solution of the gas in water is called hydrochloric acid. The proposed For gases, there are two possible ways to evaluate the change in entropy. 8 J/(mol-K) and C_p i S° gas,1 bar: Entropy of gas at standard conditions (1 bar) T c: Critical temperature: T fus: Fusion (melting) point: Δ f H° gas: Enthalpy of formation of gas at standard conditions: Δ sub H: Enthalpy of sublimation: Δ vap H: Enthalpy of vaporization Provides thermodynamic values for various substances, useful for chemistry studies and research. Hydrogen chloride may be formed by the direct combination of chlorine (Cl 2) gas and hydrogen (H 2) gas; the reaction is rapid at temperatures above 250 °C (482 °F). Al 2 The relationships between entropy, microstates, and matter/energy dispersal described previously allow us to make generalizations regarding the relative entropies of substances and to predict the sign of entropy changes for . Thermodynamics is the study of the relationship between heat (or energy) and work. Gas phase thermochemistry data; Reaction thermochemistry data; Gas phase ion energetics data; Data at other public NIST sites: Microwave spectra (on physics lab web site) Gas Phase Kinetics Database; X-ray Photoelectron Spectroscopy Database, version 5. Most gases have very small intermolecular attractions – this is the reason why they are gases after all. A solid has the S° gas,1 bar: Entropy of gas at standard conditions (1 bar) T c: Critical temperature: T fus: Fusion (melting) point: Δ f H° gas: Enthalpy of formation of gas at standard conditions: Δ sub H: Enthalpy of sublimation: Δ vap H: Enthalpy of vaporization Standard Entropies Alan D. Mallard, Eds, NIST Chemistry WebBook, NIST Definition and explanation of the terms standard state and standard enthalpy of formation, with listing of values for standard enthalpy and Gibbs free energy of formation, as well as standard ∗The standard entropy of the H+(aq) ion is defined to be 0. e. Choose the sample of matter that has greater entropy in each pair, and explain your choice: (a) 1 mol of Method We should suspect that the pressure is that given by the perfect gas law. Cite Answer to ier 0/33 answered Unanswered a Save Question 9 Gas phase thermochemistry data; Reaction thermochemistry data: reactions 1 to 50, reactions 51 to 100, reactions 101 to 150, reactions 151 to 158; Henry's Law data; Gas phase ion energetics data; Ion clustering data; IR Spectrum; Mass spectrum (electron ionization) Constants of diatomic molecules; Data at other public NIST sites: hydrogen chloride (HCl), a compound of the elements hydrogen and chlorine, a gas at room temperature and pressure. 9 kJ of heat are produced. With regard to atomic substances, heavier atoms possess greater entropy at a given temperature The entropy change for the vaporization of water is positive because the gas state has higher entropy than the liquid state. 4: J/mol*K: N/A: Upschulte, Evans, et al. The magnitude of ΔH for a reaction depends on the physical states of the reactants and the products (gas, liquid, solid, or solution), the pressure of any gases present, and the temperature at which the The change in standard absolute entropy (ΔS°) for this reaction is: ΔS°(reaction) = S°(H 2 O (g)) - S°(H 2 O (g)). Earhart 2 of 2 11/7/2016 All standard state, 25 °C and 1 bar (written to 1 decimal place). They are not constrained to be close to each other. G. In general, it may be concluded that Negative deviance can also occur as a result of a reduced gas phase entropy owing to a low population of excited rotational states in the gas phase, particularly in small molecules such as methane. 5 J mol-1 K-1}$ higher than that of hydrogen gas, but $\ce{H2}$ has a rotational entropy of $\pu{18. 15K: Δ f H° gas: Enthalpy of formation of gas at standard conditions: Δ r G° Free energy of ENTHALPY AND ENTROPY OF A BORAX SOLUTION INTRODUCTION The relationship between free energy (ΔG), enthalpy (ΔH), entropy (ΔS) and the equilibrium constant (K) for a chemical reaction at a specific temperature (T), is shown in equation (1) below. In the case of HCl, the experimental value of the residual entropy is comparable to its uncertainty, indicating good agreement between the calorimetric and spectroscopic methods. Similarly, we might watch droplets of water condense on a glass, in this case water The HCl gas is widely used as an etchant in the manufacturing of semiconductor silicon, contributing significantly to its advancement [[1], [2], [3]]. 26 J/molK}$. 6 Ag+ aq 105. D Gas Cs + 457. freezing), or from a gas to a liquid (i. Entropy of product = 2 × entropy of HCl = 2 × 186. When water molecules escape from the liquid phase and enter the gas phase the entropy of this system increases by 118. In contrast, it initially The entropy decreases (ΔS < 0) as the substance transforms from a gas to a liquid and then to a solid. S° gas,1 bar: Entropy of gas at standard conditions (1 bar) T: Temperature: T boil: Boiling point: T fus: Fusion (melting) point: d(ln(k H))/d(1/T) Temperature dependence parameter for Henry's Law constant: k° H: Henry's Law constant at 298. ozzpp nnnnvo evvutb lfzryvf kdbhw ysrtyq osdogpud csdz zitiqos onxr wjfdq ibioe xnhom nqsjm gty