Which of the following statements is (are) true? For the false statements, corre

Question

Which of the following statements is (are) true? For the false statements, correct them. At constant temperature, the lighter the gas molecules, the faster the average velocity of the gas molecules. At constant temperature, the heavier the gas molecules, the larger the average kinetic energy of the gas molecules. A real gas behaves most ideally when the container volume is relatively large and the gas molecules are moving relatively quickly. As temperature increases, the effect of interparticle interactions on gas behavior is increased. At constant V and T, as gas molecules are added into a container, the number of collisions per unit area increases resulting in a higher pressure. The kinetic molecular theory predicts that pressure is inversely proportional to temperature at constant volume and mol of gas.

Explanation / Answer

26)
Vave = sqrt (3*R*T/M)
so, smaller the value of M, greater will be Vavg
a is true

KE = 3/2 * K* T
it doesn't depend on mass
b is false

real gas behave ideally when pressure is less or volume is large and speed is large
c is true

d is true

at constant V and T
P is directly proportional to n, number of moles
e is true

P*V = n*R*T
P is directly proportional to temperature
so, f is false

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