3. The reaction, MnO:(s) + 4 HCl(aq) → MnCl:(aq) + Cl:(g) + H;O(1) was being studied. 12.2 g of MnO; were reacted with 70.0 ml of 2.50 M HCl solution. The chlorine produced was collected in a vessel. The pressure measured 0.971 atm at a temperature of 78.2 °C. Determine the volume of chlorine produced if the theoretical yield was obtained.

If 8g of ammonium hydroxide is completely decomposed by the reaction below in a closed container with a total volume of 5.00L and at 25°C, what will be the partial pressure of the ammonia gas liberated, in atmospheres? Assume the volume of the liquid is negligible. NH4OH(aq) --> H2O(l)+NH3(g)

+7 (A) 15.2 L B) 0 C) +3 D) -2 19. 68.1 g solid CaCO3 is mixed with excess HC1. What is the volume of CO2 will be collected at 0.0 °C, and 1 atm. (Molar mass CaCO3 = 100.08 g/mol, CO₂ = 44.1 g/mol CaCO3 (s) + 2 HCl(aq) → H₂O (1) +CaCl2 (aq) + CO₂(g) C) OL B) 29.9 L C D) 155 L 20. A gas sample has an initial volume of 0.500 L and initial pressure of 1.0 atm. Wha the volume when the pressure of the sample is decreased to 0.50 atm? Assume the temperature and number of moles of the gas are constant. P₁V₁ = P₂1 A) .0 L B) 0.025 L

Mg(s) + 2 HCl(aq) → MgCl2(g) + H2(g) PV = nRT R = 0.082061. 2. The volume of hydrogen gas produced was not at standard temperature and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure: STP (T = 273.15K and P = 1.00 atm). Mass of flask/stopper/5 mL H2O=112.794 g Mass of flask/stopper/filled flask of H2O=250.302 g Volume of gas space in flask (the difference between the above two measurements converted to L) =0.137508 L Trial 1: mass of Mg (g) =0.013 g pressure= 1.0104 atm temperature= 298.35 K moles of H2 =0.00054 mol