This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here's the solution for question 8: Step 1: Write the balanced chemical equation. The given reaction is: 2H_2O_2 → 2H_2O + O_2 Step 2: Relate the rates of disappearance and formation using stoichiometry. For every 2 moles of H_2O_2 that disappear, 1 mole of O_2 is formed. This means that the rate of disappearance of H_2O_2 is twice the rate of formation of O_2. Mathematically, the relationship between the rates is: -(1)/(2)d[H_2O_2]dt = d[O_2]dt Where -d[H_2O_2]dt is the rate of disappearance of H_2O_2, and d[O_2]dt is the rate of formation of O_2. Step 3: Determine the ratio of the rates. We need to find the rate of disappearance of H_2O_2 with respect to the rate of formation of O_2. This is the ratio: -d[H_2O_2]dtd[O_2]dt From the relationship in Step 2, multiply both sides by 2: -d[H_2O_2]dt = 2 × d[O_2]dt Now, divide both sides by d[O_2]dt: -d[H_2O_2]dtd[O_2]dt = 2 The ratio is 2. The correct option is A. The rate of disappearance of H_2O_2 with respect to the rate of formation of O_2 gas is A. 2. That's 2 down. 3 left today — send the next one.