Hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure
ID: 541582 • Letter: H
Question
Hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure in atmo- spheres (1 atm = 101.325 Pa = 760 torr)? 1. 2. If the atmospheric pressure in Denver is 0.88 atm then what is this in mmHg (1 atm 101,325 Pa= 760 torr, 1 torr = 1 mmHg)? 3. If 2.3 mol of a gas occupies 50.5 ml how many moles of the gas will occupy 85.5 mL at the same temperature and pressure? What is the volume of NHs produced in the following reaction when 3.0 L of Nz reacts with 4.0 L of H2? 4. N2(g) + 3H2(g) 2NH3(g) 5. A gas evolved during the fermentation of sugar was collected at 22.5°C and 702 mmHg. n its volume was found to be 25.0 L. How many moles of gas were col- lected (R- 0.08206 L atm/K mol, 1 atm 760 mmHg)? 131Explanation / Answer
1) (1atm/760torr) × 466 torr = 0.613atm
2) (760mmHg/1atm) × 0.88atm = 668.8mmHg
3) (2.3mol/50.5ml)×85.5ml = 3.89mol
4) N2(g) + 3H2(g) ------> 2NH3(g)
stoichiometrically, 1L N2 react with 3L of H2 to produce 2L of NH3
Therefore,
3L of N2 require 9L of H2 but availabe H2 is 4L
H2 is limiting
Stoichiometrically, 3L H2 produce 2L NH3
Therefore,
Volume of NH3 produced by 4L of H2 = (2/3)×4L = 2.67L
5) Ideal gas equation is
PV = nRT
no of mole, n = PV/RT
Pressure, P = 702mmHg= 0.924atm
Temperature = 22.5 = 295.7K
Volume = 25L
Therefore,
n = 0.924atm × 25L/((0.08206L atm/mol K)×295.7K)
= 0.9520mol
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