Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.32 × 10-2 M/s, what is the rate of formation of NOCl? 2 NO(g) + Cl2(g) → 2 NOCl(g)
Added by Tiffany M.
Step 1
Step 1: The rate law for the reaction with respect to Cl2 is given by rate = k[Cl2]^1. Show more…
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Reaction rate is expressed in terms of changes in concentration of reactants and products. Write a balanced equation for $$ \text {(Rate)} =-\frac{\Delta\left[\mathrm{CH}_{4}\right]}{\Delta t}=-\frac{1}{2} \frac{\Delta\left[\mathrm{O}_{2}\right]}{\Delta t}=\frac{1}{2} \frac{\Delta\left[\mathrm{H}_{2} \mathrm{O}\right]}{\Delta t}=\frac{\Delta\left[\mathrm{CO}_{2}\right]}{\Delta t} $$
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