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21 solutions

The Reaction Quotient

Q. A sample of solid I2 is present, but iodine (I) is completely absent. Given the value for Kc is 1.7x10^-3, what is the value for Q and what will happen next? I2(s) <-> 2I (g) a. Q also equals 1.7x10^-3, so there will be no change. b. Q is 0, so the reaction will shift to the right and the amount of products will increase. c. Q is 0, so the reaction will shift to the left and the amount of the reactants will increase d. Q is 0, which means that an equilibrium can never be reached e. Q cannot be determined with the information provided

Solved • Jul 25, 2019

The Reaction Quotient

Q. For the reaction below, the concentrations of HI, H2, and I2 are all 0.2 M. Which of these statements are true? 2 HI(g) <-> H2(g) + I2(g) a. The amount of products at equilibrium is greater than the amount of the reactants b. The amount of reactants at equilibrium is greater than the amount of the products. c. Q = K, so the concentrations will remain unchanged d. Since K> Q, the reaction will shift to the left to restore equilibrium. e. Since K< Q, the reaction will shift to the right to restore equilibrium.

Solved • Jul 25, 2019

The Reaction Quotient

Q. Can you explain this problem and the answers why is A ) no and and b) to the left Thank you!

Solved • Jul 21, 2019

The Reaction Quotient

Q. For the following reaction ΔHo = 2816 kJ CO2(g) + 6H2O(l)↔ 6 O2(g) + C6H12O6(s) (1) If some CO2(g)is added to the equilibrium mixture at constant temperature and volume

Solved • Jul 20, 2019

The Reaction Quotient

Q. The equilibrium constant K for this reaction at 472 celsius is 0.105: N2 (g) reacts with H2 (g) producing NH3 (g) we prepare the following mixture in one container at 472 celsius: 2.00 M H2, 1.00 M N2, and 2.00M NH3 a) is this mixture at equilibrium? how do we know if it is or not b) if not how will this mixture react to reach equilibrium ? will it shift to the right, left or no change? how do we know if it shifts to the right left or there's no change

Solved • Jul 20, 2019

The Reaction Quotient

Q. Consider the following equilibrium at 100°C. COBr2(g) - CO(g) + Br2(g) Kc = 4.74 104 (a) A system has the following concentrations at 100°C. [COBr2] = 1.69.10-6 M [CO] = 2.81 x 10-3 M [Br2] = 2.51.10-5 M Is the system at equilibrium? If not, in which direction will the reaction proceed to reach equilibrium? Ye s , the system is at equilibrium. No, the system is not at equilibrium and will shift toward the reactants. No, the system is not at equilibrium and will shift toward the products. (b) If a system has a reaction quotient of 2_1/,:1 Y----11 at 100°C, what will happen to the concentrations of COBr2, CO, and Br2 as the reaction proceeds to equilibrium? [COBr2]: decrease increase not change [CO]: decrease increase not change [Br2]: decrease increase not change

Solved • Jul 5, 2019

The Reaction Quotient

Q. For the reaction N2(g)+ 3 H2(g) - 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4.105. Use the given concentrations to determine the following. [N2]=0.0021 M [H2]=0.0048 M [NH3]=1.0e-09 M (a) Determine Q at this time. (Omit units.) (b) Determine which direction the reaction will proceed in order to reach equilibrium. left right

Solved • Jul 5, 2019