<u>Answer: </u>The correct rate of the reaction is ![Rate=k[a][b]^5[c]^6](https://tex.z-dn.net/?f=Rate%3Dk%5Ba%5D%5Bb%5D%5E5%5Bc%5D%5E6)
<u>Explanation:</u>
Rate law of the reaction is the expression which expresses the rate of the reaction in the terms of the molar concentrations of the reactants with each term raised to the power of their respective stoichiometric coefficients in a balanced chemical equation.
For the given reaction:

The expression for the rate law will be: ![Rate=k[a][b]^5[c]^6](https://tex.z-dn.net/?f=Rate%3Dk%5Ba%5D%5Bb%5D%5E5%5Bc%5D%5E6)
We are given the chemical reaction and the amount of reactant used for the process. We use these data together to obtain what is asked. We do as as follows:
0.882 mol H2O2 ( 1 mol O2 / 2 mol H2O2 ) = 0.441 mol O2 produced
Hope this answers the question.
Answer:
Explanation:
Partial pressure of oil = mole fraction of oil x total pressure
mole fraction of oil = mole of oil / mole of water + mole of oil
= mole of oil = mass of oil / molecular weight of oil
= 20 / 100 = .2
mole of water = 80 / 18
= 4.444
mole fraction of oil = .2 / .2 + 4.444
= .2 / 4.644
Partial pressure of oil = mole fraction of oil x total pressure
= (.2 / 4.644 ) x 760 mm
= 32.73 mm Hg .
Answer: It’s the first one