Please help with question 2 a-c # Prelab: Determination of Gas Law Constant R1. **Preparation** - Set up your Chem105 lab kit tub and fill it up. Be sure to let it sit overnight so the temperature stabilizes to room temperature. Tap water can go in this tub.2. **Experiment Details** - A student performed the experiment as described, using 5.00 mL of an aqueous 3.00% H₂O₂ solution, with a density of 1.101 g/mL. The water temperature was 24.0°C, and the barometric pressure was 29.34 inches of Hg. The weights of the gas-collection bottle and water were: - Partially full: 248.25g - Full: 306.03g3. **Calculations** - a. Calculate the atmospheric pressure of your environment in mmHg from a weather barometric reading. - b. Calculate the pressure exerted by the collected O₂ at the water temperature. Use the formula \( P_{\text{total}} = P_{\text{O}_2} + P_{\text{H}_2\text{O}} \) and the vapor pressure of H₂O at 24°C = 22.4 mm Hg. - c. Convert this pressure to atmospheres or kPa.### Note:- The provided weights help determine the volume of gas collected, essential for calculating the gas constant R.- Ensure all calculations consider the conversions between different units of pressure.

a.) We need to use conversion factor between inch and mm to calculate pressure in mmHg. b.) Using the total pressure and pressure of water, we can calculate pressure of O2 gas. c.) By using the conversion factor we can calculate pressure in required unit.