Study the two-steps reaction below.
Step 1 (slow): H2(g) + ICl(g) HI(g) + HCl(g)
Step 2 (fast): HI(g) + ICl(g) I2(g) + HCl(g)
Step 1 (fast): NO(g) + NO(g) N2O2(g)
Step 2 (slow): N2O2(g) + O2(g) 2NO2(g)
For each two-step reaction, answer the following:
a.Write the overall reaction. What substance is the reaction intermediate?
b.What is the rate law for the mechanism?
c.What is the molecularity of the mechanism?
The rate law or rate equation for a chemical reaction is an equation that links the initial or forward reaction rate with the concentrations or pressures of the reactants and constant parameters (normally rate coefficients and partial reaction orders).