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Multiple Choice
What is the rate law for the elementary reaction: Cl(g) + Cl(g) + N2(g) → Cl2(g) + N2(g)?
A
Rate = k[Cl][N2]
B
Rate = k[Cl2][N2]
C
Rate = k[Cl]^2
D
Rate = k[Cl]^2[N2]
Verified step by step guidance
1
Identify the elementary reaction: Cl(g) + Cl(g) + N2(g) → Cl2(g) + N2(g). This reaction involves two chlorine atoms and one nitrogen molecule as reactants.
Understand that for an elementary reaction, the rate law can be directly written from the stoichiometry of the reactants. Each reactant's concentration is raised to the power of its stoichiometric coefficient.
In this reaction, there are two Cl atoms, so the concentration of Cl should be squared in the rate law. The stoichiometric coefficient for Cl is 2.
The concentration of N2 is raised to the power of its stoichiometric coefficient, which is 1, so it appears as [N2] in the rate law.
Combine these observations to write the rate law: Rate = k[Cl]^2[N2], where k is the rate constant.