The two gas samples represented in the graph above are at the same temperature. Which of the following statements about the gases is correct?ResponsesThe molecules of gas Z have a higher average kinetic energy than the molecules of gas X.The molecules of gas Z have a higher average kinetic energy than the molecules of gas X .There are fewer molecules in the sample of gas Z than in the sample of gas X.There are fewer molecules in the sample of gas Z than in the sample of gas X .Gas Z has a smaller molar mass than gas X.Gas Z has a smaller molar mass than gas X .Gas Z has a greater molar mass than gas X.

Which statements about a sample of gas containing molecules of different masses are true?Check all that apply.You did not open hints for this part.ANSWER:More-massive gas molecules in the sample have higher rms speed than less-massive ones.The rms speed depends only on temperature, and so all types of particles in the sample have the same rms speed.More-massive gas molecules in the sample have lower rms speed than less-massive ones.

The average kinetic energy of gas molecules increases with increasing temperature.The average speed of gas molecules decreases with decreasing temperature.The temperature of a gas sample is independent of the average kinetic energy.There are gas molecules that move faster than the average.All the gas molecules in a sample cannot have the same kinetic energy.

Which gas behaves the least ideally?Multiple choice question.H2NH3HeNeAr

which parameter is same for molecules of all gases for given temperature

Which gas would occupy more volume at a constant temperature and pressure, 1.5 g of N2 gas or 1.5 g of O2 gas?A.N2 because there are more moles of N2.B.O2 because its molecules are larger.C.Neither gas occupies any volume.D.Both gases occupy equal volumes.