Question

8. In the reaction A products the initial concentration of A is 0.52M and the concentration is 0.12 M after 150.0 min. What is the value of the rate constant, k, in M min'? What is the half-life? k=0.0027 M min"!, t12=97.5 min 9. Consider the following reaction: N2(g) + 3H2(g) + 2NH3(g) (K = 2.41x 10-3) Given 2.00 mole of N2(g), 4.5 mole of H2(g), and 1.5 mole of NH3(g) are mixed in a 5.00 L flask, determine the reaction quotient, Q=0.308 Determine whether the system is in equilibrium. If not, will the concentration of NH3(g) will increase or decrease as the system reaches equilibrium? Explain your reasoning. Decrease

Answer 1

8)
a)
we have:
[A]o = 0.52 M
[A] = 0.12 M
t = 150.0 min


use integrated rate law for 0 order reaction
[A] = [A]o - k*t
0.12 = 0.52 - k*1.5*10^2
k = 2.667*10^-3 min M/min
Answer: 2.7*10^-3 min M/min

b)
Given:
k = 2.667*10^-3 M/min
use relation between rate constant and half life of 0 order reaction

t1/2 = [A]o/(2*k)
= 0.52/(2*2.667*10^-3)
= 97.5 min
Answer: 97.5 min

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