For which of the following equilibrium does K_e = K_p ? HBr(g) 1/2 H_2(g) + 1/2

Question

For which of the following equilibrium does K_e = K_p ? HBr(g) 1/2 H_2(g) + 1/2 Br_2(l) N_2(g) + 3H_2(g) 2NH_3(g) CO(g) + H_2O(g) CO_2(g) + H_2(g) CO(g) + 3H_2(g) CH_4(g) + H_2O(g) CaO(s) + CO_2(g) CaCO_3(s) The following reaction is investigated (assume an ideal gas mixture): 2N_2O(g) + N_2H_4(g) 3N_2(g) + 2H_2O(g) Initially there are 0.10 mol of N_2O and 0.25 mol of N_2H_4 in a 10.0 - L container. If there are 0.057 mol of N_2O at equilibrium, how many moles of N_2 are present at equilibrium? 1.3 times 10^-1 2.2 times 10^-2 4.3 times 10^-2 6.5 times 10^-2 none of these A reaction that is second-order in one reactant has a rate constant of 3.8 times 10^-2 L/(mol - s). If the initial concentration of the reactant it 0.260 mol/L. how long will it take for the concentration to become 0.130 180 s 18 s 1000 s 51 s 100 s At 400 K. an equilibrium mixture of H_2, I_2. and HI consists of 0.059 mol H_2, 0.075 mol I_2, and 0.12 mol HI in a 3.50-L flask. What is the value of K_p for the following equilibrium? (R = 0.0821 L middot atm/(K mol), 2 HI(g) H_2(g) + I_2(g) 8.8 0.29 28 3.4 0.036

Explanation / Answer

47)
for Kc = Kp,
number of gaseous molecules on product and reactant side should be same
which is true only for C
Answer: C

A is wrong as it has 1 gas molecule on reactant and only 1/2 in product
B is wrong as it has 4 gas molecule on reactant and only 2 in product
D is wrong as it has 4 gas molecule on reactant and only 2 in product
E is wrong as it has 1 gas molecule on reactant and only 0 in product

I am allowed to answer only 1 question at a time

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