53. At 1000 K, an equilibrium mixture in the reactionCO₂(g) + H₂(g) = CO(g) + H₂O(g) contains0.276 mol H₂, 0.276 mol CO2, 0.224 mol CO, and0.224 mol H₂O.(a) What is K at 1000 K?(b) Calculate ArGº at 1000 K.(c) In which direction would a spontaneous reactionoccur if the following were brought together at1000 K: 0.0750 mol CO₂, 0.095 mol H₂, 0.0340 mol CO,and 0.0650 mol H₂O?

The direction in which the reaction proceeds to reach equilibrium can be predicted by determining…

3. At 1000 K, an equilibrium CO₂(g) + H₂(g) — CO(g) CO(g) + 0.276 mol H₂, 0.276 mol CO2, 0.224 mol H₂O. (a) What is K at 1000 K? mixture in the reaction + H₂O(g) H₂O(g) contains 0.224 mol CO, and (b) Calculate ArGº at 1000 K. (c) In which direction would a spontaneous reaction occur if the following were brought together at 1000 K: 0.0750 mol CO₂, 0.095 mol H₂, 0.0340 mol CO, and 0.0650 mol H₂O?

3. At 1000 K, an equilibrium CO₂(g) + H₂(g) — CO(g) CO(g) + 0.276 mol H₂, 0.276 mol CO2, 0.224 mol H₂O. (a) What is K at 1000 K? mixture in the reaction + H₂O(g) H₂O(g) contains 0.224 mol CO, and (b) Calculate ArGº at 1000 K. (c) In which direction would a spontaneous reaction occur if the following were brought together at 1000 K: 0.0750 mol CO₂, 0.095 mol H₂, 0.0340 mol CO, and 0.0650 mol H₂O?

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

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
The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) +You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, andthe concentration of NH3 is 0.85 M.(a) Calculate the value of the reaction quotient Q.(b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed toreach equilibrium.
The equilibrium constant for the following reaction is 20.9 at 907 °C. 2 SO2(g) + O2(g) 2 SO3(g) K= 20.9 at 907 °C Calculate the equilibrium constant for the following reactions at 907 °C. (a) 2 SO3(g) 2 SO2(g) + 02(g) K= (b) SO3(g) SO (g) + 1/2 O2(g) K=
For this equilibrium system, 2SO3(g) 2 25O2(g) + O2(g), Kc = 0.00407. At equilibrium, you would expect to find %3D relatively more products than reactant. relatively more reactant than products. about comparable amounts of reactant and products. no way to decide.
Methanol, CH3OH, is manufactured industrially by the reaction CO(g) + 2H2 (g) = CH3OH(g) A gaseous mixture at 500 K is 0.020M CH3OH, 0.10MCO, and 0.10MH2. What will be the direction of reaction if this mixture goes to equilibrium? The equilibrium constant Ke equals 10.5 at 500 K.
At -7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction. Here are some facts about the reaction: • The constant pressure molar heat capacity C, 1.76 J·mol -1. K¯!. • If the reaction is run at constant pressure, the volume increases by 14.%. The initial rate of the reaction is 11. mol·L - 1 -1 •S O Yes. Using these facts, can you calculate K, at 15. °C? O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K at Yes, and K, will be 15. °C will be bigger or smaller than K, at -7.73 °C? smaller.
Nitrogen and hydrogen react to form ammonia, like this: N2 (g)+3H,(g) 2NH;(g) Suppose a mixture of N,, H, and NH, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. alo perturbation change in composition shift in equilibrium Ar to the right The pressure of N, will to the left Some H, is removed. The pressure of NH, will (none) to the right The pressure of N, will ? to the left Some NH, is added. The pressure of H, will v ? O (none) go up. go down. not change.
13) Consider the reaction between nitrogen and steam: 2N₂(g) + 6H₂0(g) ⇒ 4NH3(g) + 30₂(g) At a certain temperature, K = 28.6. Calculate the equilibrium partial pressure of steam if PNH₂ = 1.75 atm, Po₂ = 0.963 atm, and P№₂ = 0.996atm at equilibrium.
When 0.200 mol of CaCO,(s) and 0.300 mol of CaO(s) are placed in an evacuated, sealed 10.0-L container and heated to 385 K, PCO, = 0.220 atm after equilibrium is established. 2 CACO,(s) = CaO(s) + CO,(g) Additional CO,(g) is pumped into the container to raise the pressure to 0.470 atm. After equilibrium is re-established, what is the total mass (in g) of CaCO, in the container?
The following reaction takes place into a constant-volume flask at 427°C: CCL(g) = C(s) +2 C2(g) AH=132 kJ At 427°C, the equilibrium constant for the reaction given above is K. = 1.3×10-2. A flask is filled with 2.00 atm of CCl4 at 427°C. (a) What is the value of K for this reaction? (R=0.082 L.atm/mol.K) (b) What are the partial pressures of CClL, Ch and the total pressure at equilibrium? (c) How will the equilibrium pressure of CCl(g) change if the temperature is increased? (d) How will the equilibrium system respond if the volume of the flask is reduced?
Kp for the following reaction is 0.16 at 25 0C. 2NOBr(g)=2NO (g)+ Br2 (l) the enthalpy change for the reaction at standard conditions is +16.1 kJ. State which way the equilibrium will shift (left, right or no change) when each of the following changes is made. Breifly explain credit for result. (a) adding more Br2 (l) (b) removing some NOBr (g) (c) Decreasing the temperature (d) increasing the container volume (e) increasing the total pressure by adding an inert gas.
Consider the following equilibrium for which H = 180.74: N2(g) + O2(g) 2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system. (b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f) O2(g) is removed from the system.