Chapter 8, Problem 8.63UTC

Two flasks of equal volume and at the same temperature contain different gases. One flask contains 10.0 g of Ne, and the other flask contains 10.0 g of He. Is each of the following statements true or false? Explain. (8.1)

1. The flask that contains He has a higher pressure than the flask that contains Ne.
2. The densities of the gases are the same.

Interpretation Introduction

To determine:

Whether the given statement is true or false

Answer to Problem 8.63UTC

The statement is true.

Explanation of Solution

The statement is the flask that contains He has a higher pressure than the flask containing Ne

Given: Two flasks with same volume and same temperature contain two different gases. One flask contains 10 g Ne and other flask contains 10 g He.

Formula used: PV = nRT where P, V, T, n and R are pressure, volume, temperature, mole of gas and universal gas constant respectively.

Calculation: 10 g Ne = $\frac{10}{20}$ mole = 0.5 mole and 10 g He = $\frac{10}{4}$ moles = 2.5 moles

Pressure of He gas containing flask = $\frac{nRT}{V}=\frac{2.5\times R\times T}{V}$

Pressure of Ne containing gas = $\frac{0.5\times R\times T}{V}$

Thus pressure of the flask containing He gas is more than that of Ne.

Conclusion

The given statement is true.

Interpretation Introduction

To determine:

Whether the given statement is true or false

Answer to Problem 8.63UTC

The statement is true.

Explanation of Solution

The statement given is the densities of the gases are same.

Given: Two flasks with same volume and same temperature contain two different gases. One flask contains 10 g Ne and other flask contains 10 g He.

Formula used: $\text{density}\text{=}\frac{\text{Mass}}{\text{Volume}}$

Calculation:

$\text{density}\text{=}\frac{\text{Mass}}{\text{Volume}}$

Since, the mass and volume of the two gases are same so, the densities of the gases are the same.

Conclusion

The given statement is true.