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Calculate the pressure that CCl4 will exert at 40 C if
Chapter , Problem 10.96(choose chapter or problem)
Calculate the pressure that CCl4 will exert at 40 C if 1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys the idealgas equation; (b) CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are given in Table 10.3.) (c) Which would you expect to deviate more from ideal behavior under these conditions, Cl2 or CCl4? Explain
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QUESTION:
Calculate the pressure that CCl4 will exert at 40 C if 1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys the idealgas equation; (b) CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are given in Table 10.3.) (c) Which would you expect to deviate more from ideal behavior under these conditions, Cl2 or CCl4? Explain
ANSWER:Problem 10.96 Calculate the pressure that CCl4 will exert at 40 if 1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys the ideal gas equation; (b) CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are given in Table 10.3.) (c) Which would you expect to deviate more from ideal behavior under these conditions, Cl2 or CCl4 Explain Step-by-step solution Step 1 of 4 Given data: Moles of CCl 4g), n = 1.00 mol Volume of the gas, V = 33.3 L Temperature of gas, T = 40 = (40 + 273) K = 313 K a) The ideal gas equation is: PV = nRT …… (1) Here, R is gas constant = 0.08206 L-atm/mol-K Solving the equation (1) for P and substituting in the known values gives: nRTP = V = (1.00 mol)(0.08206 Latm/molK)(313 K) 33.3 L = 0.771 atm So, the pressure exerted by CCl (g4 is 0.771 atm.