An ideal gas, initially at a pressure of 10.3 atm and a temperature of 312 K, is allowed to expand adiabatically until its volume doubles.   What is the gas’s final temperature, in kelvin, if the gas is monatomic?  What is the gas’s final pressure, in atmospheres, if the gas is diatomic?

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What is the average energy per molecule of a gas at 592 K? unit J %3D Assuming the gas is 02, has a molecular mass of 32 u, what is the rms speed of each molecule? unit

An insulated container contains two moles of an ideal gas at atmospheric pressure. Keeping the pressure constant, if the temperature of the gas is increased by 50 °C, then its volume increases by 400 cm3 and if the temperature is increased by 100 °C, then its volume increases by 600 cm³. Determine the initial volume and temperature of the gas. (Write the equation of ideal gas initially, after the temperature increase of 50 °C, and after increase of temperature by 100 °C. Combine these three equations to find the initial volume and temperature)

Three moles of an ideal gas at 135C and 0.5 atm is allowed to expand 1 atm at a constant pressure to a volume twice as large. What is the new temperature?

Problem #1: An ideal gas of initial volume V=1m^3, initial temperature T=1000C and initial pressure P=10,000 Pa is heated up to a final temperature T=3000C and allowed to expand into a final volume V=3m^3. What is the final pressure?

2.00 mol of helium and 1.00 mol of argon are separated by a very thin barrier. Initially the helium has 7500 J of thermal energy. The helium gains 2500 J of energy as the gases interact and come to thermal equilibrium by exchanging energy via collisions at the boundary. What was the initial temperature of the argon? First, what is the equilibrium temperature of the two gases? Express your answer in kelvins. ► View Available Hint(s) Tf = Submit Part B VE ΑΣΦ help What is the thermal energy of the argon at the equilibrium temperature? Express your answer with the appropriate units.