The equation for a reversible reaction used in industry to convert methane to hydrogen is shownbelow. CH4(g) + H2O(g) → CO(g) + 3H2(g), AH = +210 kJ. Which statement is always correct about this reaction when equilibrium has been reached? The concentrations of methane and carbon monoxide are equal. The amount of hydrogen is three times the amount of methane. The value of AH for the reverse reaction is -210 kJ. The rate of the forward reaction is greater than the rate of the reverse reaction.

The equation for a reversible reaction used in industry to convert methane to hydrogen is shownbelow. CH4(g) + H2O(g) → CO(g) + 3H2(g), AH = +210 kJ. Which statement is always correct about this reaction when equilibrium has been reached? The concentrations of methane and carbon monoxide are equal. The amount of hydrogen is three times the amount of methane. The value of AH for the reverse reaction is -210 kJ. The rate of the forward reaction is greater than the rate of the reverse reaction.

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

1. 2NO(g) + O₂(g) ⇒ 2NO₂(g) Consider the reaction Which would decrease the partial pressure of NO₂(g) at equilibrium? A) Increasing the volume of the system B) Adding a noble gas to increase the pressure of the system C) Adding NO(g) to the system D) Adding an appropriate catalyst E) Decreasing the volume of the system for which ΔΗ<0.
Answer the following questions based on the given information about this chemical reaction.
Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature. A. 2Cl2O(g) → 2Cl2(g) + O2(g) ΔH°rxn = –151 kJ B. 3O2(g) → 2O3(g) ΔH°rxn = +284 kJ C. COCl2(g) → CO(g) + Cl2(g) ΔH°rxn = +112 kJ D. 2C(s) + 2S(s) + O2(g) → 2COS(g) ΔH°rxn = –137 kJ E. N2O4(g) → 2NO2(g) ΔH°rxn = +171 kJ
The following reaction is product-favored at equilibrium at room temperature. C,H2 (g) + H2 (g) → C,H4 (g) Will raising or lowering the temperature make it reactant-favored? Raising the temperature can make it reactant-favored. O Lowering the temperature can make it reactant-favored. O Neither raising nor lowering the temperature can make it reactant-favored.
Consider the following equilibrium: 2NO, (g) – N,04(g) AG = - 5.4 kJ Now suppose a reaction vessel is filled with 7.26 atm of dinitrogen tetroxide (N,O) at 95. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can that yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,0, 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. atm Round your answer to 2 significant digits. O O
For the following reaction, AH = 2816 kJ. 6 CO₂(g) + 6 H₂O(I) ⇒ C6H12O6(s) + 6 O₂(g) Select ONE combination of strategies that when applied to this system at equilibrium will result in an increase in the amount of C6H₁2O6 as equilibrium is re-established? a. Increasing Po₂ by adding more O2; increasing the temperature; decreasing the volume; or removing CO₂ b. Increasing Po₂ by adding more O₂ and decreasing the volume C. Decreasing the volume d. Increasing Po₂ by adding more O₂ e. Increasing the temperature
For the reaction below, what is the effect of raising the temperature? 4A(g) + B(g) 3C(g) AH = - 405 kJ Equilibrium shifts to the right; the reaction makes more products. O The reaction makes more of both products and reactants, so equilibrium is unaffected O Equilibrium re-establishes Equilibrium shifts to the left; the reaction makes more reactants.
17. The thermochemical equation for the reaction of F2 and water is as follows. AH = -270 kJ F2(g) + 2 H2O (liq)=HF (aq) + O2 (g) Given a system that is initially at equilibrium, which of the following actions cause the reaction to proceed to the right? a) adding O2(g) b) decreasing the temperature c) adding a catalyst d) decreasing the volume of the reaction chamber e) none of the above
Consider the following equilibrium: N₂ (g) + 3H₂(g)2NH₂ (g) AG = -34. KJ 2 Now suppose a reaction vessel is filled with 3.70 atm of hydrogen (H₂) and 8.46 atm of ammonia (NH3) at 1099. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of H ₂ tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding N₂? x Ś ? In other words, if you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the yes no pressure of H₂ will tend to fall, can that be changed to a tendency to rise 2 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. atm Round your answer to 2 significant digits. ● O
Consider the reaction A →B with AH° = 60.55 kJ/mol,xn and the reaction B -→C with AH = 65.96 kJ/molxn- What should be the AH° in kJ/moln for the reaction A+ C→ 2 B? Report your answer to three decimal places.
The standard reaction free energy AG° = - 190. kJ for this reaction: CH3OH(g) + CO(g) -»HCH3CO2(l) Use this information to complete the table below. Round each of your answers to the nearest kJ.