Question

Lab Activity - Kinetics NAME: \( \qquad \) 1. Nitrogen monoxide reacts with chlorine according to the equation: \[ 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NOCl}(g) \] The following initial rates of reaction have been observed for certain reactant concentrations: \begin{tabular}{|c|c|c|} \hline\( [\mathrm{NO}](\mathrm{mol} / \mathrm{L}) \) & {\( \left[\mathrm{Cl}_{2}\right](\mathrm{mol} / \mathrm{L}) \)} & Rate \( \left(\mathrm{mol} \mathrm{L}^{-1} \mathrm{~h}^{-1}\right) \) \\ \hline 0.50 & 0.50 & 1.14 \\ \hline 1.00 & 0.50 & 4.56 \\ \hline 1.00 & 1.00 & 9.12 \\ \hline \end{tabular} a) Write the rate law expression for the reaction. b) Determine the rate order for NO with respect to \( \mathrm{Cl}_{2} \) ? c) What is the rate order for \( \mathrm{Cl}_{2} \) with respect to NO ? d) What is the rate constant, \( k \) ? e) Finaly, what is the rate law for the reaction? Include the orders with respect to each reactants and \( k \) ?

          Lab Activity - Kinetics

NAME: \( \qquad \)
1. Nitrogen monoxide reacts with chlorine according to the equation:
\[
2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NOCl}(g)
\]

The following initial rates of reaction have been observed for certain reactant concentrations:
\begin{tabular}{|c|c|c|}
\hline\( [\mathrm{NO}](\mathrm{mol} / \mathrm{L}) \) & {\( \left[\mathrm{Cl}_{2}\right](\mathrm{mol} / \mathrm{L}) \)} & Rate \( \left(\mathrm{mol} \mathrm{L}^{-1} \mathrm{~h}^{-1}\right) \) \\
\hline 0.50 & 0.50 & 1.14 \\
\hline 1.00 & 0.50 & 4.56 \\
\hline 1.00 & 1.00 & 9.12 \\
\hline
\end{tabular}
a) Write the rate law expression for the reaction.
b) Determine the rate order for NO with respect to \( \mathrm{Cl}_{2} \) ?
c) What is the rate order for \( \mathrm{Cl}_{2} \) with respect to NO ?
d) What is the rate constant, \( k \) ?
e) Finaly, what is the rate law for the reaction? Include the orders with respect to each reactants and \( k \) ?

Lab Activity - Kinetics

NAME:
1. Nitrogen monoxide reacts with chlorine according to the equation:

2 NO(g)+Cl2(g) ⟶ 2 NOCl(g)

The following initial rates of reaction have been observed for certain reactant concentrations:

[NO](mol / L) [Cl2](mol / L) Rate (molL^-1 h^-1)

0.50 0.50 1.14

1.00 0.50 4.56

1.00 1.00 9.12

a) Write the rate law expression for the reaction.
b) Determine the rate order for NO with respect to Cl2 ?
c) What is the rate order for Cl2 with respect to NO ?
d) What is the rate constant, k ?
e) Finaly, what is the rate law for the reaction? Include the orders with respect to each reactants and k ?

Added by Stephen C.

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