A 1.50 L gas cylinder contains a mixture of nitrogen gas (N 2 ) and hydrogen gas (H 2 ) at a temperature of 35.0oC and a pressure of 895 torr. What is the pressure in atmospheres (atm)? b. What is the...

A 1.50 L gas cylinder contains a mixture of nitrogen gas (N 2 ) and hydrogen gas (H 2 ) at a temperature of 35.0oC and a pressure of 895 torr. What is the pressure in atmospheres (atm)? b. What is the pressure in pounds per square inch (psi)? c. If the partial pressure of N 2 is 615 torr, what is the partial pressure of H2? d. If the temperature is increased to 70.0oC, what is the new partial pressure of each gas and what is the new total pressure? e. How many moles of N 2 and moles of H 2 are present in the cylinder? f. How many grams of N 2 and grams of H 2 are present in the cylinder? g. How many molecules of N 2 and molecules of H 2 are present in the cylinder? h. Nitrogen gas and hydrogen gas react according to the equation: N 2 (g) + 3H 2 (g) ? 2NH 3 (g) Assuming that conditions in the cylinder allow the reaction to take place, which is the limiting reactant, N 2 or H 2 ? i. For the reaction in part h, what is the theoretical yield (in grams) of NH3?