### Calculating the Equilibrium Constant for the Hydrogenation of Acetylene#### Problem DescriptionCalculate the equilibrium constant, \( K \), at 25.0 °C for the hydrogenation of acetylene to ethane, using the thermodynamic information provided in the table.#### Chemical ReactionThe balanced chemical equation for the hydrogenation of acetylene (C₂H₂) to ethane (C₂H₆) is as follows:\[ \text{C}_2\text{H}_2 (g) + 2 \text{H}_2 (g) \rightleftharpoons \text{C}_2\text{H}_6 (g) \]#### Required FormulaThe equilibrium constant \( K \) can be calculated from the standard Gibbs free energy change \( \Delta G^\circ \) using the formula:\[ \Delta G^\circ = -RT \ln K \]Where:- \( R \) is the gas constant, 8.314 J/(mol·K)- \( T \) is the temperature in Kelvin (298.15 K for 25.0 °C)#### Thermodynamic DataThe following table provides the standard Gibbs free energy of formation \( \Delta G_f^\circ \) for each compound involved in the reaction:| Compound | \( \Delta G_f^\circ \) (kJ · mol⁻¹) ||----------------|--------------------------------------|| CH₃Cl(g) | 48.50 || CH₄(g) | -50.72 || C₂H₂(g) | 209.2 || C₂H₆(g) | -32.82 || Cl₂(g) | 0.00 || H₂(g) | 0.00 || H₂O(l) | -237.13 || HCl(g) | -95.30 || HNO₃(aq) | -111.25 || NO(g) | 86.55 || NO₂(g) | 51.31 |#### Steps to Calculate \( \Delta G^\circ \) for the Reaction1. **Identify Products and Reactants:** - Products: C₂H₆(g) - Reactants: C₂H₂(g),

∆rG° = free energy of formation of products - free energy of formation of reactants∆rG° = - RTlnK T…

Calculate the equilibrium constant, K, at 25.0 °C for each of the reactions. Use the thermodynamic information provided in the table. The hydrogenation of acetylene to ethane. C,H,(g) +2H,(g) →C,H(g) K = x10 TOOLS Compound CH₂Cl(g) CH₂(g) C₂H₂(g) C₂H6 (g) Cl₂(g) H₂(g) H₂O(1) HCl(g) HNO₂ (aq) NO(g) NO₂ (g) AG; (kJ. mol-¹) 48.50 -50.72 209.2 -32.82 0.00 0.00 -237.13 -95.30 -111.25 86.55 51.31

Calculate the equilibrium constant, K, at 25.0 °C for each of the reactions. Use the thermodynamic information provided in the table. The hydrogenation of acetylene to ethane. C,H,(g) +2H,(g) →C,H(g) K = x10 TOOLS Compound CH₂Cl(g) CH₂(g) C₂H₂(g) C₂H6 (g) Cl₂(g) H₂(g) H₂O(1) HCl(g) HNO₂ (aq) NO(g) NO₂ (g) AG; (kJ. mol-¹) 48.50 -50.72 209.2 -32.82 0.00 0.00 -237.13 -95.30 -111.25 86.55 51.31

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following equilibrium: N₂O₂ (g) 2NO₂ (g) 2 AG=5.4 kJ Now suppose a reaction vessel is filled with 2.57 atm of dinitrogen tetroxide (N₂O4) at 138. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. rise fall O yes no 10 FAED alo Ar
At 13.7 °C the concentration equilibrium constant K = 2.0 × 10 for a certain reaction. Here are some facts about the reaction: • C The constant pressure molar heat capacity C₁ = 2.49 J-mol K. •If the reaction is run at constant pressure, 147. kJ/mol of heat are released. •If the reaction is run at constant pressure, the volume increases by 13.%. ○ Yes. Using these facts, can you calculate K, at 3.8 °C? x10 No. If you said yes, then enter your answer at right. Round it to 2 significant digits. n If you said no, can you at least decide whether Kat 3.8 °C will be bigger or smaller than K at -13.7 °C? Yes, and K will be bigger. Yes, and K will be smaller. No. x
Calculate the value of K, for the equation C(s) + CO₂(g) given that at a certain temperature Kp = 2 CO(g) K₂ = ? C(s) + 2 H₂O(g) CO₂(g) + 2 H₂(g) H₂(g) + CO₂(g) = H₂O(g) + CO(g) Kpl = 3.35 Kp2 = 0.745
Give typed explanation of both otherwise leave it Not a single word hand written otherwise leave it
The synthesis of CaCO3 uses this chemical reaction. CaO(aq) + CO2(g) ——> CaCO3(s) + 180 kJ Identify three stresses that can be imposed on the equilibrium to maximize the amount of CaCO3 present. Be specific about what, if any, compounds are involved in those stresses.
What would happen to the (i) equilibrium constant, K, of the following reactions and the (ii) direction of equilibrium shift upon heating?
Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm X S
Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Ś
Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D
Please don't provide handwritten solution ....
Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5
Consider the following equilibrium: 2NH3(g) → N₂(g) + 3H₂(g) AG = 34. kJ Now suppose a reaction vessel is filled with 6.39 atm of ammonia (NH3) and 0.200 atm of hydrogen (H₂) at 206. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. OO U rise fall yes no atm x10 X Ś