Chapter 5: Q5.30P (page 228)

You have 357 mL of chlorine trifluoride gas at 699 mmHg and $45 ° C$ . What is the mass (in g) of the sample?

Short Answer

Expert verified

Answer

The mass of the gas is 1.165 g.

Step by step solution

Ideal gas law

The ideal gas law equation is,

$P V = n R T$

The ideal gas law for the given condition can be written as,

$n = \frac{PV}{RT}$

Here,

V is the volume (375 mL)

T is the temperature ( $45 ° C$ ).

P is the pressure (699 mmHg).

Determination of mass

Before putting the values, we need to convert the given units in desired units,

$V = 375 m L = 375 m L \times \frac{1 L}{10^{3} m L} = 0.375 L$

And,

$T = 45 ° C = 45 + 273 = 318 K$

And,

$760 m m H g = 1 a t m 699 m m H g = 699 m m H g \times \frac{1 a t m}{760 m m H g} 699 m m H g = 0.919 a t m$

The number of moles of gas in the sample is,

$n = \frac{PV}{RT} n = \frac{0.919 atm \times 0.375 L}{0.0821 {atmLK}^{- 1} {mol}^{- 1} \times 318 K} n = 0.0126 m o l$

The molar mass of chlorine trifluoride is $92.45 g / m o l$ .

The mass of the sample is,

$M a s s = m o l e s \times m o l a r m a s s = 0.0126 m o l \times 92.45 g / m o l = 1.165 g$

Thus, the mass of the gas is 1.165 g.

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You have 357 mL of chlorine trifluoride gas at 699 mmHg and $45 ° C$ . What is the mass (in g) of the sample?

Short Answer

Step by step solution

Ideal gas law

Determination of mass

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You have 357 mL of chlorine trifluoride gas at 699 mmHg and 45°C. What is the mass (in g) of the sample?

Short Answer

Step by step solution

Ideal gas law

Determination of mass

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Kinetics

Chemical Analysis

Chemical Reactions

Organic Chemistry

Ionic and Molecular Compounds

Study anywhere. Anytime. Across all devices.

You have 357 mL of chlorine trifluoride gas at 699 mmHg and $45 ° C$ . What is the mass (in g) of the sample?