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Question

# 6.   Using your answer from Question 5 and assuming that the decomposition of

H2O2 into oxygen was complete, how many moles of H2O2 did you start with? Show your work and include units.

﻿﻿ 2H2O2 (aq) –> 2H2O(l) + O2(g)

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This is the question I’m having trouble with I’m not sure exactly how I should go about doing this problem? Like formula wise. Below is my work for question 5

5.   Using the Ideal Gas Law along with your answer in Question 4 and your data in Table 1, what quantity of oxygen (in moles) was liberated from your hydrogen peroxide? Show your work and include units.

N= P V / R T

(1.03atm)(47.9mL) / (0.0821)(294.85K)=

=49.337/24.207

=2.04mol