nitrosyl bromide, NOBr is formed from NO and Br2-. Experiments show that this reaction is second order in NO and first order in Br2.
what is the rate equation for this reaction?
rate = k(NO)^2(Br)
what is the initial rate of the reaction, in mol/(L*s) under these conditions?
Concentration= 0.40 mol/L
The rate equation for this reaction can be determined by the powers to which the reactants are raised. The given information states that the reaction is second order in NO and first order in Br2.
Therefore, the rate equation can be written as:
Rate = k[NO]^2[Br2]
Where:
- Rate is the rate of the reaction,
- k is the rate constant,
- [NO] represents the concentration of NO,
- [Br2] represents the concentration of Br2.
To determine the rate equation for a reaction, we need to analyze the experimentally obtained reaction orders of the reactants. In this case, the reaction is second order in NO and first order in Br2.
The rate equation is generally expressed in the form: Rate = k[A]^m[B]^n, where k is the rate constant, [A] and [B] are the concentrations of reactants, and m and n are the respective reaction orders.
Given that the reaction is second order in NO and first order in Br2, we can express the rate equation as: Rate = k[NO]^2[Br2]^1.
Therefore, the rate equation for this reaction is Rate = k[NO]^2[Br2].