Question

The Volume of 2.8 g CO at 27 degree C and 0.821 atm pressure is (R = 0.08210 Lit. atm $\text{K}^{-1} \text{mol}^{-1}$)

• A. 3 litres
• B. 0.3 litres
• C. 30 litres
• D. 1.5 litres

Answer 1

Answer: (A)

3 litres

Answer 2

To determine the volume of CO (carbon monoxide) gas at the given conditions, we can use the ideal gas law equation:
$PV = nRT$
First, we need to convert the temperature from Celsius to Kelvin:
$T(K) = T(C) + 273.15$
$T(K) = 27 + 273.15 = 300.15 K$
Next, we can calculate the number of moles of CO:
$n = \frac{\text{mass}}{\text{molar mass}}$

$n = \frac{2.8 \, \text{g}}{12.01 \, \text{g/mol} + 16.00 \, \text{g/mol}}$

$n = \frac{2.8 \, \text{g}}{28.01 \, \text{g/mol}}$
n = 0.099964 mol (approximately 0.1 mol)
Now, we can substitute the values into the ideal gas law equation:
$PV = nRT$

$V = \frac{{nRT}}{{P}}$

$V = \frac{{(0.1 \, \text{mol})(0.08210 \, \text{L atm K}^{-1} \, \text{mol}^{-1})(300.15 \, \text{K})}}{{0.821 \, \text{atm}}}$
V = 3.007 L (approximately 3 L)
Therefore, the volume of 2.8 g of CO at 27 degrees Celsius and 0.821 atm pressure is approximately (A) 3 litres.