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Chapter 5: Q5.27P (page 228)

A sample of carbon monoxide occupies 3.65 L at 298 K and 745 torr. Find its volume at $- 14 掳 C$ and 367 torr.

Short Answer

Expert verified

Answer

The final volume is 6.44 L.

Step by step solution

01

Ideal gas law

The ideal gas law equation is,

$P V = n R T$

The ideal gas law can also be written as,

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

(Moles of the sample are fixed)

02

Determination of final volume

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Here,

$V_{1}$ is the initial volume (3.65 L).

$V_{2}$ is the final volume.

$T_{1}$ is the initial temperature (298 K).

$T_{2}$ is the final temperature (259 K).

$P_{1}$ is the initial pressure (745 torr).

$P_{2}$ is the final pressure (367 torr).

The final volume of the given sample at STP is,

$V_{2} = \frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}} V_{2} = \frac{745 torr 脳 3.65 L}{298 K} 脳 \frac{259 K}{367 torr} V_{2} = 6.44 L$

Thus, the final volume is 6.44 L.

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Most popular questions from this chapter

A 75.0-g sample of dinitrogen monoxide is confined in a 3.1-L vessel. What is the pressure (in atm) at $115 掳 C$ ?

Why is moist air less dense than dry air?

Convert the following:

(a) 0.745 atm to mmHg (b) 992 torr to bar

(c) 365 kPa to atm (d) 804 mmHg to kPa

Convert each of the pressures described below to atm:

(a) At the peak of Mt. Everest, atmospheric pressure is only $2.75 脳 10^{2} 鈥� m m H g$ .

(b) A cyclist fills her bike tires to $86 鈥� p s i$ .

(c) The surface of Venus has an atmospheric pressure of $9.15 脳 10^{6} 鈥� P a$ .

(d) At 100 ft below sea level, a scuba diver experiences a pressure of $2.54 脳 10^{4} 鈥� t o r r$ .

A gas-filled weather balloon with a volume of 65.0 L is released at sea-level conditions of 745 torr and $25 掳 C$ . The balloon can expand to a maximum volume of 835 L. When the balloon rises to an altitude at which the temperature is $鈭� 5 掳 C$ and the pressure is 0.066 atm, will it reach its maximum volume?

See all solutions

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