Question: When a lab assistant tried to buy a cylinder of hydrogen for his experiments, he found the follow…
Show transcribed image text When a lab assistant tried to buy a cylinder of hydrogen for his experiments, he found the following information on the data sheet: Internal volume of the cylinder: 34 L; mass of hydrogen: 1.00 kg. (9](a) Assuming hydrogen under this condition behaves as an ideal gas, please calculate the pressure exerted by hydrogen molecules inside such a cylinder at 20 degreeC. (9](b) You probably have noticed that the pressure you calculated in [9](a) is very high, and therefore hydrogen may not behave as an ideal gas. Johannes van der Waals won the Nobel prize in physics in 1910 "for his work on the equation of state for gases and liquids". Let's calculate the pressure exerted by H_2 inside such a cylinder at 20 degreeC using the van der Waals equation, given that for H_2, a = 0.2444 atm L^2 mol^-2, and b = 0.02661 L mol^-1. [9](c) Please compare your answers in [9](a) and (9](b) and decide whether the attractions or repulsions between O_2 molecules dominate at these conditions. Please clearly state your reasoning. (9](d) The compressibility factor z is defined as z = PV/nRT. Please calculate the compressibility factor of hydrogen at these conditions. We have learnt in lecture that repulsive forces increase z, whereas attractive forces reduce z. Does your answer in [9](d) agree with that in [9](c)? (No need to explain here.)
When a lab assistant tried to buy a cylinder of hydrogen for his experiments, he found the following information on the data sheet: Internal volume of the cylinder: 34 L; mass of hydrogen: 1.00 kg. (9](a) Assuming hydrogen under this condition behaves as an ideal gas, please calculate the pressure exerted by hydrogen molecules inside such a cylinder at 20 degreeC. (9](b) You probably have noticed that the pressure you calculated in [9](a) is very high, and therefore hydrogen may not behave as an ideal gas. Johannes van der Waals won the Nobel prize in physics in 1910 "for his work on the equation of state for gases and liquids". Let's calculate the pressure exerted by H_2 inside such a cylinder at 20 degreeC using the van der Waals equation, given that for H_2, a = 0.2444 atm L^2 mol^-2, and b = 0.02661 L mol^-1. [9](c) Please compare your answers in [9](a) and (9](b) and decide whether the attractions or repulsions between O_2 molecules dominate at these conditions. Please clearly state your reasoning. (9](d) The compressibility factor z is defined as z = PV/nRT. Please calculate the compressibility factor of hydrogen at these conditions. We have learnt in lecture that repulsive forces increase z, whereas attractive forces reduce z. Does your answer in [9](d) agree with that in [9](c)? (No need to explain here.)
