[ask] How to calculate the initial rates of the reaction 2NO + Cl2 => 2NOCl?

Thread starter pengko
Start date Mar 5, 2007
Tags

Initial Reaction

AI Thread Summary

To calculate the initial rates of the reaction 2NO + Cl2 => 2NOCl, one can use the rate law, which typically involves the concentrations of the reactants. The initial rate can be expressed as a function of the concentrations of NO and Cl2 raised to their respective reaction orders. It is important to determine the order of the reaction experimentally, which can be done through initial rate experiments. The discussion emphasizes the need for a clear understanding of how to apply rate equations to this specific reaction. Accurate calculations require knowledge of the stoichiometry and the relationship between concentration and rate.

Mar 5, 2007

pengko

Does anyone know how to calculate the initial rates of the reaction 2NO + Cl2 => 2NOCl? Using the initial rates of NO or Cl2? Thanks a lot for the respond =)

Physics news on Phys.org

Mar 6, 2007

chemisttree

Science Advisor

Homework Helper

Gold Member

Please show us your initial attempt.

What equations for rate of reaction do you know? How might they be applied to answer this problem?

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...

View full post »