For which of the following systems at equilibrium and at constant temperature wi

Question

For which of the following systems at equilibrium and at constant temperature will decrease the volume cause the equilibrium to shift to the righr? NH_4Cl(s) NH_2(g) + HCl(g) H_2(g) + Cl_2(g) 2HCl(g) 2H_2O(g) 2H_2(g) + O_2(g) 2NO_2(g) 2NO(g) + O_2(g) N_2(g) + 3H_2(g) 2NH_3(g) For which of following reaction are the numerical values of K_p and K the same? 2SO_2(g) + O_2(g) 2SO_2(g) N_2(g) + O_2(g) 2NO(g) H_2(g) + I_2(g) 2HI(g) 2 only 1, 2, and 3 2 and 3 only 1 only 1 and 2 only Consider the following equilibrium: C_2H_6(g) + C_5H_12 (g) CH_4(g) + C_6H_14(g); K_p = 9.57 at 500K. Suppose 11.9 g each of CH_4, C_2H_6, C_5H_12, and C_6_14 are placed in a 50.0-L reaction vessel at 500 K. What is the value of Q_p? 0.104 0.637 1.00 9.57 1.57 Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to the following equation: 2NO + 2H_2 rightarrow N_2 + 2H_2O The experimental rate taw is Rate = k[NO]^2[H_2]. If time is measured in minutes and concentration is measured in moles per liter, what are the units for the rate of production of nitrogen. mol^2/(L^2 middot min). mol^3/(L^3 middot min). mol/(L^2 middot min). L^2/(mol^2 middot min). mol/(L middot min). Which of the following corresponds to the correct integrated expression for a first-order reaction? 1/A - 1/A_0 = kt 1/A_0 - ln A/A_0 = kt ln A - ln A_0 = -kt t_1/2 = 0.693/k 1/A - 1/B = kt At a given temperature, a first-order reaction has a rate constant of 2.0 times 10^-3 s^-1. How long will it take for the reaction to be 33% complete? 1700 s 550 s 87 s 2100 s 200 s In a first-order reaction, the half-life is 125 minutes. What is the rate constant? 5200 s^-1 0.333 s^-1 1.33 times 10^-4 s^-1 5 54 times 10^-3 s^-1 9.24 times 10^-5 s^-1

Explanation / Answer

32)
decreasing volume will move the reaction where there are less gaseous molecules
Only E has lesser number of molecules on product side as compare to that on reactant side
hence Answer is E

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