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Chapter 5: Q5.30P (page 228)

You have 357 mL of chlorine trifluoride gas at 699 mmHg and 45掳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

01

Ideal gas law

The ideal gas law equation is,

PV=nRT

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

n=PVRT

Here,

V is the volume (375 mL)

T is the temperature (45掳C).

P is the pressure (699 mmHg).

02

Determination of mass

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

V=375mL=375mL脳1L103mL=0.375L

And,

T=45掳C=45+273=318K

And,

760mmHg=1atm699mmHg=699mmHg脳1atm760mmHg699mmHg=0.919atm

The number of moles of gas in the sample is,

n=PVRTn=0.919atm脳0.375L0.0821atmLK-1mol-1脳318Kn=0.0126mol

The molar mass of chlorine trifluoride is 92.45g/mol.

The mass of the sample is,

Mass=moles脳molarmass=0.0126mol脳92.45g/mol=1.165g

Thus, the mass of the gas is 1.165 g.

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