Question

15. A-D

Gas name: Acetylene

15. A chemist wishes to study (get your gas name below) at high pressures and low temperatures. A. Why are these conditions where a gas would act nonideally? B. Use the ideal gas law to calculate the number of moles of your gas required to produce a pressure of 200.0 atm in a 2 L container at 200.0°C above your gases boiling point. C. Repeat the calculation in part a, but use the van der Waals equation to obtain a more accurate value. This may need to be solved iteratively. To solve this equation iteratively, ask your instructor how. Your answer for the number of moles correct to 4 significant figures. D. What is the percent error in the ideal gas law estimate? (Assume that the van der Waals value is correct.) 000 must be If your last name starts with (L'atm/mol) b(L/mol Compound Acetic acid Acetic anhydride Acetone Acetonitrile Acetylene Ammonia Ar Benzene Bromobenzene 0.1068 0.1263 0.0994 0.1 I 68 17.82 20.16 14.09 17.81 4.4480.05136 4.225 1.363 0.03219 18.24 28.94 0.03707 0.1154 0.1539 I, J 35

Answer 1

(a) condition for a gas would act as non-ideally (1) At high pressure the gas molecules get clase very much each other so the space between the molecule is reduced and the force of attraction between the molecule is increased (2) At low temperature, the thermal energy of molecule is decreased which also increases the crowdness between the molecular increases Therefore they also induce same vander waal interaction due to claseness between the molecules (b) Ideal gas law pv = nRT p material implication pressure of the gas p = 200.0 atm v material implication volume of the system v = 2.00l n material implication no. of moles of gas R material implication gas constant T material implication temperature T = 200 degree c T = 200 + 273.15 = 473.15 k n = PV/RT material implication (200 atm)(2.00 l)/(0.0821 l atm kt mol^-1)(473.15k) n = 10.29 mol (c) vander waal equation (p + n^2a/V_m^2)(v-nb) = RT for acetylene gas a = 4.448 l^2 atm/mal^2 b = 0.05136 l/mol (200 + n^2(4.448 l^2 atm/mol^2)/(2l)^2)(2-0.0136n)