Step-by-step explanation:
H2 (g) + 2NO(g) → N2O(g) + H2O(g)
Trial 1 Trial 2 Trial 3
H2 (M) 0.30 0.60 0.60
NO (M) 0.35 0.35 0.70
Rate (M*s) 2.835 x 10^-3 1.134 x 10^-2 2.268 x 10^-2
a. What is the order with respect to H2?
Comparing trial 1 and 2, the conc of H2 is doubled, the rate of the reaction increased by a factor f 4. This means the rate is in second order with respect to H2.
b. What is the order with respect to NO?
Comparing Trial 2 and 3, the concentration of NO is doubled, the rate of the reaction increased by a factor of 2. This means the rate is in first order with respect to NO.
c. What is the rate equation for this reaction?
The rate equation is given as;
rate = k [H2]²[NO]
d. Calculate the rate constant for the reaction.
Taking trial 1;
2.835 x 10^-3 = k (0.30)²(0.35)
k = 2.835 x 10^-3 / 0.0315 = 90 x 10^-3
k = 0.09 L2 mol-2 s-1