Part A The average rate of the reaction between 10 and 20 s. Express your answer

Question

Part A The average rate of the reaction between 10 and 20 s. Express your answer using two significant figures. Rate = M?s?1

Part B The instantaneous rate of the reaction at 30 s. Express your answer using two significant figures.

Part C The instantaneous rate of formation of O2 at 50 s. Express your answer using two significant figures.

Part D If the initial volume of the H2O2 solution is 1.2 L , what total amount of O2(in moles) is formed in the first 50 s of reaction? Express your answer using two significant figures.

Explanation / Answer

Part A:

-dA/dt = r

r = -(0.55 - 0.75) / 20 - 10 = 0.020 M/s

Part B:

r = 0.4 / 30 = 0.013 M/s

Part C:

r = 0.22 / 50 = 0.0044 M/s

Part D:

initial moles of H2O2 = V* M = 1.2 * 1 = 1.2 moles

at the end of 50 s ,

concentration 0f H2O2 = 0.2 M

so, moles of H2O2 = V* M = 1.2 * 0.2 = 0.24 moles

moles of H2O2 used = 1.2 - 0.24 = 0.96 moles,

2 moles of H2O2 produces 1 mol of O2 ,
so ,
0.96 moles of H2O2 will produce: 0.96 / 2 = 0.48 moles of O2

Hope this helps

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