The figure shows a pV diagram for 0.0066 mol of gas that undergoes the process 1 → 2 → 3.What is the pressure p₂.The ideal gas constant is R = 8.314 J/mol • K = .

Question

Quizplus · Accepted Answer

The pressure at point 1 can be found by dividing the product of the initial pressure and volume by the final volume (Boyle's Law). Using the given graph, the volume at point 1 is approximately 1.2 L and the final volume is 2.4 L. Therefore, the pressure at point 1 is (2 atm * 1.2 L)/2.4 L = 1 atm. Next, we can use the ideal gas law to find the temperature at point 1. Assuming the gas is ideal, we can use the formula PV = nRT, where n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. At point 1, we have P = 1 atm, V = 1.2 L, n = 0.0066 mol, and R = 8.314 J/mol*K. Solving for T gives T = (1 atm * 1.2 L)/(0.0066 mol * 8.314 J/mol*K) = 219 K. Using this temperature and the final volume of 2.4 L, we can find the pressure at point 2 using the formula P1V1/T1 = P2V2/T2 (Gay-Lussac's Law). Plugging in the values we know, we get P2 = (1 atm * 1.2 L * 219 K)/(0.0066 mol * 2.4 L) = 22.1 atm. Finally, we can use the graph to find the pressure at point 3, which is approximately 16 atm. Therefore, the pressure values for the three points are: P1 = 1 atm P2 = 22.1 atm P3 = 16 atm The question is asking for the pressure at point ₂, which is the same as the pressure at point 2. The answer is A) 5.3 atm, which is the closest to 22.1 atm.

The Figure Shows a PV Diagram for 0