Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC2(s) + 2H2O(l) -> C2H2(g) + Ca(OH)2(aq) The product gas, C2H2, is collected over water at a temperature of 20 °C and a pressure of 754 mm Hg. If the wet C2H2 gas formed occupies a volume of 5.69 L, the number of grams of C2H2 formed is _________ g. The vapor pressure of water is 17.5 mm Hg at 20 °C.

Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCl(aq) → ZnCl₂ (aq) + H₂(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 752.0 mm Hg. If the wet H₂ gas formed occupies a volume of 7.62 L, the number of grams of H₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.

11. In the early study of air composition, Ramsey in 1894 separated water vapor, nitrogen, oxygen and carbon dioxide from air by absorption processes. Lord Rayleigh separated these gases by a different process. Both men were left with a small amount of gas with a density of 1.63 g/L at 25 °C and 1 atm. Which element did they discover?

Consider the reaction below which was carried out at 200.0 K to produce liquid ammonia: N2(8) + 3H,(g) 2NH3() Suppose 37.3 g of N2 gas is mixed with 37.3 g of H2 gas. What is the volume (in units of liters) of gas remaining after the reaction is completed? The remaining gas was measured to have a temperature of 200.0 K and a pressure of 760.0 mmHg? molar mass of N2= 28.013 g/mol molar mass of H2 = 2.0158 g/mol. %3D Recall: Vo (1/P) (at constant Tand n) VaT (at constant P and n) Van (at constant Tand P) PV = nRT rate of effusion ox 1 atm 760 torr 760 mmHg %3D %3D R=8.31446 J K-1.r mol-1 R= 0.0820573L atm K-1. mol-1 %3D