and neon atoms to 2 significant figures. 15. Consider two gases, A and B, each i

Question

and neon atoms to 2 significant figures. 15. Consider two gases, A and B, each in a 1.0 L. container and each at the same temperature and pressure. The mass of gas A in the container is 0.54 g and the mass of gas B in the container is 0.40 g 0.54 g 0.40 g a. Which container has more molecules? b. Which gas sample has the largest average kinetic energy? c. Which gas sample has the fastest average velocity? d. The molecules A are larger than B and thus hit the walls with more force, so how can the pressure in the two containers be equal to each other? 16. Nitrogen gas (N,) reacts with hydrogen gas (H,) to form ammonia gas (NH,). You have nitrogen nd hydmren gases in a 18.0 L container fitted with a movable piston (the piston moves so as to nf each reactant gas

Explanation / Answer

(A)

Use ideal has eqaution.

PV= nRT

here T is same, P is same and also V is same for both gas. R is a constant.

therefore n1=n2   => no. of moles of both gas are same

1. they both have same no. of molecules.

2. avg. kinetic energy = KbT/2 same for both gas.

3.calculating average velocity :

vavg = (2RT/M)1/2 , where,

vavg = average velocity

R = gas constant ( 8.314 J/K)

T = absolute temperature

M = molar mass.

Assuming that both gases are in equimolar amount , since mass of A is less , so its molar mass is also less than B

We have seen that the average velocity is inversely proportional to mass

Thus , average velocity of A is more than that of B.

4. pressure is force/ area = (N/3)(mv2/l3)

here though m is greater for gas b. v2 variers as inverse of m. Hence they balance each other and pressure remains constant.

The heavier Gas A molecules collide more forcefully, but gas B molecules have a faster average velocity and collide more frequently.

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