how would you do 9a? this is a non graded practice worksheet **Problem 9: Decomposition of Hydrogen Peroxide**Hydrogen peroxide is a common compound that readily decomposes if left out for too long. In this experiment, a sample of the aqueous solution decomposes, and the oxygen produced is collected via water displacement using a gas collection tube. The collected data is displayed in the table below.**Chemical Reaction:**\[ 2 \text{H}_2\text{O}_2 (\text{aq}) \rightarrow 2 \text{H}_2\text{O} (\text{l}) + \text{O}_2 (\text{g}) \]**Data:**| Parameter | Value ||-------------------------------|-------------|| Atmospheric Pressure | 758.99 torr || Temperature | 22.8°C || Vapor Pressure of Water (at 22.8°C) | 20.815 torr || Volume of Gas Collected | 193.6 mL |**Questions:**a. What is the partial pressure of \(\text{O}_2 (\text{g})\) produced in the decomposition?b. How many moles of \(\text{O}_2 (\text{g})\) were produced in the decomposition?c. Calculate the experimental mass of \(\text{H}_2\text{O}_2\) that would need to decompose in order to form this amount of oxygen.

According to Dalton's Law of Partial Pressure states that the total pressure exerted by a mixture of two or more non-reacting gases is equal to the sum of the individual partial pressures which each gas would exert if it occupies the same volume alone at a constant temperature.0.9713 atm0.00774 moles0.526 g