Answer to Question #138494 in Physical Chemistry for Aashuu

Question

Write the rate of reaction in terms of the rate of disappearance of reactant and the
rate of formation of products:
1. NO(g)+O3(g)→NO2(g)+O2(g)
2. 2C2H6(g)+7O2(g)→4CO2(g)+6H2O(aq)
3. H2(g)+I2(g)→2HI(g)
4. 4OH(g)+H2S(g)→SO2(g)+2H2O(aq)+H2(g)

Answer 1

Rate (r) law equations are below. The derivatives with minus are disappearence rates of reactants, the derivatives with plus are the formation rates of products; k are rate constants, a and b are reaction orders by appropriate reactants:

1. r = -d[NO(g)]/dt = -d[O3(g)]/dt = d[NO2(g)]/dt = d[O2(g)] = k*[NO(g)]^a*[O3(g)]^b

2. r = -d[C2H6(g)]/2dt = -d[O2(g)]/7dt = d[CO2(g)]/4dt = d[H2O(aq)]/6dt = k*[C2H6(g)]^a*[O2(g)]^b

3. r = -d[H2(g)]/dt = -d[I2(g)]/dt = -d[HI(g)]/2dt = k*[H2(g)]^a*[I2(g)]^b

4. r = -d[OH(g)]/4dt = -d[H2S(g)]/dt = d[SO2(g)]/dt = d[H2O(aq)]/2dt = d[H2(g)]/dt = k*[OH(g)]^a*[H2S(g)]^b