Answer:
A. I and V
Explanation:
According to Le Chatelier's Principle, increasing the product side will cause the equilibrium to shift back towards the reactant side, so I is true. By the same principle, II is false.
For gases, decreasing the pressure will cause the equilibrium to shift towards the side with higher number of moles. So V is true.
The reaction is endothermic, so increasing the temperature will shift the equilibrium to the products, so IV is false. And adding a catalyst has no effect on the equilibrium, so III is false.
Answer:
Explanation:
a) 1.00 - 0.12 = 0.88
m = 1200(0.88)^t
b) t = ln(m/1200) / ln(0.88)
c) m = 1200(0.88)^10 = 334.20 g
d) t = ln(10/1200) / ln(0.88) = 37.451... = 37 s
e) t = ln(1/1200) / ln(0.88) = 55.463... = 55 s
B. Starting with most recent