Based on the answers to the following questions what would be the answer to the resulting question. Calculations: 1.Write the balanced equation for the reaction conducted in this lab, including appropriate phase symbols. Mg(s) + 2 Hl (aq) → MgCl(aq) +H2(g) 2Determine the partial pressure of the hydrogen gas collected in the gas collection tube. 22.4torr (1atm / 760torr) = 0.0295atm. 1.10atm – 0.0295 = 1.0705atm. 3Calculate the moles of hydrogen gas collected. n=PV/RT = 1.0705atm(0.0322L) / (0.0821Latm/molK x 297K) = 0.00141mol H2 4 If magnesium was the limiting reactant in this lab, calculate the theoretical yield of the gaseous product. Show all steps of your calculation. 0.034gMg (1molMg/24.3gMg)(1molH2 / 1molMg)= 0.00140mols 5 Determine the percent yield of this reaction, showing all steps of your calculation. yield = (.001413/.068)(10) Would the following errorsincrease,decrease, or haveno effecton the calculated moles of gas collected in the experiment? Explain your answers in complete sentences. The measured mass of the magnesium was smaller than the true mass. The actual temperature of the hydrogen gas is lower than room temperature. Explain in terms of particle collisions and Dalton’s law why it can be assumed that the total pressure inside the gas collection tube is equal to the atmospheric pressure outside of the tube. If an undetected air bubble was trapped inside the gas collection tube, how would this affect your calculated percent yield? Explain your answer.