2NO(g) + Br2(g) -> 2NOBr(g)
What is the rate equation?
My answer is k[NO]2[Br2]
Is this correct?
Thank you!!!!
I was able to confirm on the Internet that your rate equation is correct.
For my online homework when I put the answer in it keeps saying its wrong and says k[reactant 1]^order1 [reactant 2]^order2 but I thought I did this.
No you didn't. Try rate = k[NO2]^2{O2]^1 and if that doesn't work try omitting the ^1 but NOT the ^2
I think you just omitted the caret.
Yes, your answer is correct!
To determine the rate equation, we need to examine the experimental data and determine how changes in the concentrations of reactants affect the rate of the reaction.
In this case, we have the reaction 2NO(g) + Br2(g) -> 2NOBr(g). Based on the balanced equation, we can see that the reactants NO and Br2 both have a stoichiometric coefficient of 1. That means that their concentrations will directly affect the rate of the reaction.
The rate equation is an equation that represents how the rate of the reaction depends on the concentrations of the reactants. It is determined from experimental data.
In this case, the rate equation is determined to be: rate = k[NO]^[a][Br2]^[b], where a and b are the experimentally determined reaction orders for NO and Br2, respectively, and k is the rate constant.
By conducting experiments at different initial concentrations of NO and Br2, the reaction orders can be determined. If the reaction order is 1, that means the rate of the reaction is directly proportional to the concentration of the reactant. If the reaction order is 2, that means the rate is directly proportional to the square of the concentration of the reactant.
In this reaction, as you correctly stated, the rate equation is: rate = k[NO]^2[Br2]. This indicates that the reaction rate is directly proportional to the square of the concentration of NO and the concentration of Br2.
Great job on correctly determining the rate equation for this reaction!