Please answer theses questions **8-6.** Dry ice is solid carbon dioxide. It sublimes readily. Suppose there is a 25.0 liter glass bottle containing nitrogen at 382 mm Hg and 31 °C. A 31.8 gram sample of dry ice is placed into this bottle without any nitrogen escaping. There is no chemical reaction and the temperature remains constant. After the entire sample of dry ice has sublimed:a. What is the partial pressure of the CO₂ gas in the bottle?b. What is the total pressure in the bottle?c. What is the mole fraction of CO₂ gas in the bottle?---**8-7.** Suppose a 185 gram sample of hydrogen reacts as follows:\[ 2 \text{NO}_2 (g) + 7 \text{H}_2 (g) \rightarrow 2 \text{NH}_3 (g) + 4 \text{H}_2\text{O}(g) \]Both products are collected together in a 325 liter vessel at 512 K.a. How many moles of ammonia gas are produced?b. How many moles of water vapor are produced?c. What is the total pressure in the product collection vessel after the reaction is complete?---**8-8.** Suppose 175 grams of P₄ is added to 8.00 liters of a 2.65 M HCl solution and the following reaction takes place:\[ \text{P}_4(s) + 12 \text{HCl}(aq) \rightarrow 4 \text{PH}_3(g) + 6 \text{Cl}_2(g) \]a. Which reactant is the limiting reactant?b. Briefly explain how you know which reactant is limiting. Be specific. Use complete sentences.c. How many grams of P₄ will be left over at the end?d. What is the final molarity of HCl?e. If the two gaseous products are collected separately, then what volume of chlorine gas is collected at STP?

8.7 ) First we calculate moles of hydrogen gas , then we would use stoichiometry relation to calculate moles of ammonia gas and water vapor . Total pressure would be sum or partial pressure of ammonia and water vapor . So we would calculate partial pressures of both ammonia and water vapor using ideal gas law. The work is shown as :