no need for solution just answer all directly 1 for the following reaction2 no5g 4no2go2gthe ini

1. For the elementary unimolecular process, Rate of reaction = k[O2][O].

No need for solution just answer all directly 1 for the...

For the following reaction: 2 NO5(g) -> 4 NO2(g) + O2(g), the initial rate of formation of O2 was found to be 1.25 x 10-4 mol dm-3 s-1. What is the initial rate of consumption of N2O5? A) 2.50 x 10-4 mol dm-3 s-1 B) 1.25 x 10-4 mol dm-3 s-1 C) 3.75 x 10-4 mol dm-3 s-1 D) 5.00 x 10-4 mol dm-3 s-1 2. Which of the following expressions describes the rate of reaction for the elementary unimolecular process: O3 -> O2 + O? A) Rate of reaction = k[O2][O] B) Rate of reaction = k[O] C) Rate of reaction = k[O]3 D) Rate of reaction = k[O2]2[O] 3. For the following elementary reaction: HF + NH3 -> F- + NH. The rate of consumption of the reactants and rate of formation of products is given by which set of expressions? A) d[HF]/dt = -k[HF] d[NH3]/dt = -k[NH3] d[F-]/dt = k[F-] d[NH]/dt = k[NH] B) d[HF]/dt = -k[HF] d[NH3]/dt = -k[NH3] d[F-]/dt = -k[F-] d[NH]/dt = -k[NH] C) d[HF]/dt = k[HF] d[NH3]/dt = k[NH3] d[F-]/dt = -k[F-] d[NH]/dt = -k[NH] D) d[HF]/dt = k[HF] d[NH3]/dt = k[NH3] d[F-]/dt = k[F-] d[NH]/dt = k[NH]

Transcript

00:01 Dear students, the question is here on this equation nitrogen reacts with oxygen to form n2o3, rate of disappearance of nitrogen is given 3 atmosphere per minute and we have to calculate rate of formation or appearance of n2o3 gas.

00:19 So, let us see rate of disappearance also we can write minus dn2 divided by dt, this is also known as rate of disappearance, rate of disappearance of nitrogen which is 3 atmosphere per minute.

00:47 So, we have to find out rate of appearance that is d of n2o3 divided by dt, this we have to find out.

00:59 Now, if from the balanced equation rate equal to, rate of reaction equal to minus 1 by 2 dn2 divided by dt equal to, taking oxygen it is minus one -third, the coefficients will become here, so equal to minus one -third do2 by dt equal to plus 2 means half dn2o3 divided by dt, 2 is the coefficient here, n is the coefficient here, 2 is the coefficient of nitrogen.

01:45 Now, we need to relate this to nitrogen with n2o3, so relating this to rate of appearance d of n2o3 divided by dt is will be bringing to this side or 2, 2 cancels out minus dn2 by dt.

02:05 So, here if we bring to this side, 2, 2 will cancel out that means rate of appearance or formation of n2o3 is equal to rate of disappearance of nitrogen which is given 3 atmosphere per minute and this is the answer.

02:24 The second part of the question says, what is the rate of overall pressure change in the reaction chamber? now, we observed here, rate of disappearance of nitrogen is equal to rate of appearance of n2o3, therefore these two will balance each other because rate of disappearance is 3 atmosphere per minute and rate of appearance of n2o3 is also 3 atmosphere per minute, therefore they will balance each other.

02:52 But rate of disappearance of oxygen, we are getting it is 3 by 2 of rate of disappearance of nitrogen which is equal to 3 by 2, 3 by 2 multiplied by 3 equal to 9 by 2 equal to 4 .5 atmosphere per minute.

03:19 Therefore, it is clear that the overall pressure change is 3 .4 atmosphere per minute because the pressure change by decreased by nitrogen will be compensated by pressure increased by formation of n2o3 and only oxygen pressure change will affect the overall pressure change, therefore it is 4 .5 atmosphere per minute.

03:44 Now, the next part of the question here is, draw an energy versus reaction coordinate diagram to explain how can a catalyst slows down a chemical reaction, that means it is a inhibitor, the catalyst is a inhibitor not a promoter.

04:04 So, here reaction progress and here it is energy, now this is the draw an energy versus reaction coordinate diagram to explain how can a catalyst slows down a chemical reaction.

04:24 Now, you see before addition of the catalyst, let this be the reactants and let this be the products, now before addition of the catalyst, let the energy diagram is like this, so here this is the activation energy...

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