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)

Suppose you have 0.53 moles of an ideal gas. What is the average kinetic energy of that gas (in units of kJ) if the temperature of the gas is 280.2K? Note: It is understood that the unit of your answer is some number of kilo-Joules, however do not explicitly include units in your answer. Enter only a number. If you do enter a unit ("kJ" in this case), you answer will be counted wrong.

Two glass containers, of equal volume each hold a mole of gas. Container 1 is filled with hydrogen gas (molar mass 2 g / mol), and Container 2 holds helium (molar mass 4 g / mol). If the pressure of the gas in Container 1 equals the pressure of the gas in Container 2, which of the following is true?   (a)  The temperature of the gas in Container 1 is lower than the temperature of the gas in Container 2. (b)  The temperature of the gas in Container 1 is greater than the temperature of the gas in Container 2. (c)  The value of R for the gas in Container 1 is ½ the value of R for the gas in Container 2. (d)  The rms speed of the gas molecules in Container 1 is lower than the rms speed of the gas molecules in Container 2. (e)  The rms speed of the gas molecules in Container 1 is greater than the rms speed of the gas molecules in Container 2.

Consider two containers with the same volume and temperature.   The first container is labelled "Dry" and holds "dry" air = a ratio of nitrogen (N2) and oxygen (O2). The second container is labelled "Humid" and holds "moist" air = the SAME ratio of nitrogen and oxygen, but also contains water (H2O) vapor. According to the ideal gas law, if the pressures are equal, the weight of the gas inside the "Dry" container will be

(a) The temperature of a gas increases from 40.5 K to 73.5 K while its volume remains constant. What is the new pressure? Give your answer as a multiple of the initial pressure P (b) The temperature of a gas increases from 40.5 C to 73.5°C while its volume remains constant. What is the new pressure? Give your answer as a multiple of the initial pressure Pr- Pi

If I contain 3 moles of gas in a container with a volume of 60 liters and at a temperature of 400 K, what is the pressure inside the container?

(6) There is a cylindrical container with a piston with diameter d: volume to change. Sitting on top of that piston is a m = the diatomic gas is T 4.67cm which allows the 6.62kg block. The temperature of 382K and there are N 1.45 x 1023 molecules. || (a) What is the gauge pressure of the gas inside the container? (b) What is the volume of this container in cm³? (c) What is the mean free path of a molecule in this container? (d) When the block is remo sure matches external air pressure. How much distance will the piston move during this expansion? (e) What is the work done on this gas by the surroundings while the piston moves to its new position? noved, the gas will expand isothermally until the internal pres-

REAL GASES n=1 mol of real gas is in a container with a volume of v=0.25lt. The pressure of the gas at T1=300K temperature is p1=90atm, and at T2=350K the pressure of the gas is P2=110atm. Find the Vanderwaals constants (a and b) for this gas.

n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.135 m3   Part (a)  The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas?        Part (b)  The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas

2.40 moles of an ideal gas is initially at 40.0 oC and 1.35 atm. a) What is its volume under these conditions?b) If it is then compressed to one third of its initial volume and its pressure increases to 2.0 atm, what, in Centigrade degrees, will be its temperature?