Consider the reaction:
2 N2O( g) ¡ 2 N2( g) + O2( g)
a. Express t...

Question

Consider the reaction:
2 N2O( g) ¡ 2 N2( g) + O2( g)
a. Express the rate of the reaction in terms of the change in
concentration of each of the reactants and products.

Accepted Answer

Hey everyone in this example, we need to determine the expression for the reaction rate. Using the change in concentration of our reactant and products. So we're given a equation for the synthesis of ammonia gas and we should recall that for our rate expression, we're going to say our rate is equal to the change in concentration of our first reacting and two gas divided by the change in time. And it's going to be multiplied by its coefficient. So we have a coefficient of one according to our reaction and this is going to be a negative value due to the fact that we will be losing this since it's a reactant. So moving forward, we have the next part of our rate constant Or rate expression rather where we have the change in concentration of our second react in H2 gas divided by the change in time. Where we're going to multiply by the following coefficient, which according to the equation, we have a coefficient of three in front of our H2 gas and this should be in the denominator. So we would have negative 1/3 because we're losing this since it's a reactant. So that's our coefficient and then we're gonna set this equal to the change in concentration of our ammonia, which will be over our change in time. And we're going to multiply this by a coefficient of we have to according to our equation. So we should have a coefficient of one half which is positive here. Since this is a reactant that we will gain or a sorry, product that we will gain. And so to complete this example, this entire expression we've written out is going to be our final example for our rate expression so and just so that this is here. So I hope that everything I've read was clear. If you have any questions, please leave them down below and I will see everyone in the next practice video.

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