For the reaction X+Y-Z, K = 100. If the initial concentrations of X, Y, and Z are 0.8, 0.1 and 8 M respectively, which of the following will happen and why? The amounts of X and Y will decrease as more Z forms, because Q is less than K. The amounts of X and Y will decrease as more Z forms, because Q is greater than K. The amount of Z will decrease as more X and Y form, because Q is less than K The amounts of X, Y, and Z will remain the same, because Q is already equal to K O The amount of Z will decrease as more X and Y form, because Q is greater than K.

For the reaction X+Y-Z, K = 100. If the initial concentrations of X, Y, and Z are 0.8, 0.1 and 8 M respectively, which of the following will happen and why? The amounts of X and Y will decrease as more Z forms, because Q is less than K. The amounts of X and Y will decrease as more Z forms, because Q is greater than K. The amount of Z will decrease as more X and Y form, because Q is less than K The amounts of X, Y, and Z will remain the same, because Q is already equal to K O The amount of Z will decrease as more X and Y form, because Q is greater than K.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 55QRT

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Similar questions

The equilibrium constant Kc for the reaction PCl3(g)+Cl2(g)PCl3(g) equals 4.1 at 300C. a A sample of 35.8 g of PCl5 is placed in a 5.0-L reaction vessel and heated to 300C. What are the equilibrium concentrations of all of the species? b What fraction of PCl5 has decomposed? c If 35.8 g of PCl5 were placed in a 1.0-L vessel, what qualitative effect would this have on the fraction of PCl5 that has decomposed (give a qualitative answer only; do not do the calculation)? Why?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three experiments are done at different temperatures and equilibrium concentrations are measured. For each experiment, calculate the equilibrium constant, Kc. (a) [A] = 0.74 mol/L, [B] = 0.74 mol/L (b) [A] = 2.0 mol/L, [B] = 2.0 mol/L (c) [A] = 0.01 mol/L, [B] = 0.01 mol/L What can you conclude about this statement: If the concentrations of reactants and products are equal, then the equilibrium constant is always 1.0.
An equilibrium mixture of dinitrogen tetroxide, N2O4, and nitrogen dioxide, NO2, is 65.8% NO2 by mass at 100 atm pressure and 25C. Calculate Kc at 25C for the reaction N2O4(g)2NO2(g)
A vessel originally contained 0.0200 mol iodine monobromide (IBr), 0.050 mol I2, and 0.050 mol Br2. The equilibrium constant Kc for the reaction I2(g)+Br2(g)2IBr(g) is 1.2 102 at 150C. What is the direction (forward or reverse) needed to attain equilibrium at 150C?
The equilibrium constant (Kc) for this reaction is 5.0 at a given temperature. CO(g)+H2O(g)CO2(g)+H2(g) (a) On analysis, an equilibrium mixture of the substances present at the given temperature was found to contain 0.20 mol of CO, 0.30 mol of water vapor, and 0.90 mol of H2 in a liter. How many moles of CO2 were there in the equilibrium mixture? (b) Maintaining the same temperature, additional H2 was added to the system, and some water vapor was removed by drying. A new equilibrium mixture was thereby established containing 0.40 mol of CO, 0.30 mol of water vapor, and 1.2 mol of H2 in a liter. How many moles of CO2 were in the new equilibrium mixture? Compare this with the quantity in part (a), and discuss whether the second value is reasonable. Explain how it is possible for the water vapor concentration to be the same in the two equilibrium solutions even though some vapor was removed before the second equilibrium was established.
Phosgene, COCl2, used in the manufacture of polyurethane plastics, is prepared from CO and Cl2. CO(g)+Cl2(g)COCl2(g) An equilibrium mixture at 395C contains 0.012 mol CO and 0.025 mol Cl2 per liter, as well as COCl2 If Kc at 395C is 1.23 103, what is the concentration of COCl2?
A container with a volume of 1.500 L was evacuated and then filled at low temperature with 0.0500 mol liquid dinitrogen tetroxide, N2O4. As the temperature was raised, this substance formed nitrogen dioxide, NO: N2O4(g)2NO2(g) If the pressure of this reaction mixture at equilibrium at 25.0C was 0.971 atm, what was the total moles of gas in this mixture? What are the moles of NO2 and moles of N2O4? What are the partial pressures of NO2 and N2O4? What is Kc at 25.0C?

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