Question

An engineer pumps 5.00 mol of carbon monoxide gas into a cylinder that has a capacity of 20.0L. What is the pressure In kPa of gas inside the cylinder at 25 °C?

*use the ideal gas law*

Answer 1

Answer: The pressure of the cylinder is 619.1 kPa

Explanation:

To calculate the pressure, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = ?

V = Volume of the gas = 20.0 L

T = Temperature of the gas = $25^oC=[25+273]K=298K$

R = Gas constant = $8.31\text{L kPa }mol^{-1}K^{-1}$

n = number of moles of CO gas = 5.00 moles

Putting values in above equation, we get:

$P\times 20.0L=5.00mol\times 8.31\text{ L. kPa }mol^{-1}K^{-1}\times 298K\\\\P=\frac{5.00\times 8.31\times 298}{20.0}=619.1kPa$

Hence, the pressure of the cylinder is 619.1 kPa

Answer 2

The pressure In KPa of the carbon monoxide gas inside the cylinder at 25 °C is 619.393 KPa

Data obtained from the question

• Number of mole (n) = 5 moles
• Volume (V) = 20 L
• Temperature (T) = 25 °C = 25 + 273 = 298 K
• Gas constant (R) = 8.314 L.KPa/Kmol

• Pressure (P) =?

How to determine the pressure

The pressure of the carbon monoxide gas in the cylinder can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

Divide both side by V

P = nRT / V

P = (5 × 8.314 × 298) / 20

P = 619.393 KPa

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