The initial temperature of three moles of oxygen gas is 33.5°C, and its pressure is 7.80 atm. (a) What will its final temperature be when heated at constant volume so the pressure is two times its initial value? °C (b) Now the volume of the gas is also allowed to change. Determine the final temperature if the gas is heated until the pressure and the volume are doubled. °C
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- The temperature at state A is 20.0ºC, that is 293 K. How many moles of ideal gas is there in the container? 1.00 atm = 1.00×105 Pa. Your answer needs to have 3 significant figures, including the negative sign in your answer if needed. Do not include the positive sign if the answer is positive. No unit is needed in your answer, it is already given in the question statement.A tank contains one mole of nitrogen gas at a pressure of 5.20 atm and a temperature of 24.5°C. The tank (which has a fixed volume) is heated until the pressure inside triples. What is the final temperature of the gas? °C (b)A cylinder with a moveable piston contains one mole of nitrogen, again at a pressure of 5.20 atm and a temperature of 24.5°C. Now, the cylinder is heated so that both the pressure inside and the volume of the cylinder double. What is the final temperature of the gas? °CThe total translational kinetic energy of the molecules of a sample of gas at 455 K is 10500 J. How many moles n does the sample comprise? n = mol Find the average translational kinetic energy Kav of a single molecule. Kay = J
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