This is my 2nd time posting this question: please help me! Suppose you carried o

Question

This is my 2nd time posting this question: please help me!

Suppose you carried out the decomposition reaction using 20.0 mL of reaction solution (i.e. 10.0 mL of 6.1% hydrogen peroxide and 10.0 mL of the solvent, water). Assume that you observed the pressure increase by 0.128 atm over a period of 15.0 seconds at a constant temperature, 22.5oC.

Molar to pressure conversion factor is 0.041

A. How many moles of oxygen gas are produced in 15.0 seconds? Hint: Use your mole-to-pressure change ratio calculated in 1B.

B. What would be the concentration of oxygen (in molarity units) if the gas had remained in the solution?

C. Based on the above data, what is the rate of formation of oxygen (in units of molarity per second)? What is the rate of the reaction? (different than the formation of oxygen)?

PLEASE HELP using the appropriate units and steps. I appreciate it and thank you in advance! I am just having trouble with setting up the problems for some reason!

Explanation / Answer

A) From the conversion factor, we determine the moles of O2 formed:

Moles O2 = 0.128 atm * (0.041 molar / 1 atm) = 0.005248 moles

B) Calculating Molarity of O2 in 20 mL of solution:

[O2] = 0.005248 moles / 0.02 L = 0.2624 M

C) Calculating O2 formation rate:

Rate = 0.2624 M / 15 s = 0.0175 M / s

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