One mole of CO2(g) occupies 0.382 × 10−3 m³ at 40°C. Calculate the pressure that the gas would exert assuming…

Question

One mole of CO2(g) occupies 0.382 × 10−3 m³ at 40°C. Calculate the pressure that the gas would exert assuming ideal behavior. Take R = 8.314 J·mol⁻¹·K⁻¹.

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One mole of $\text{CO}_{2(g)}$ occupies $0.382 \times 10^{-3} \text{ m}^3$ at $40^\circ\text{C}$ . Calculate the pressure that the gas would exert assuming ideal behavior. Take $R = 8.314 \text{ J} \cdot \text{mol}^{-1} \cdot \text{K}^{-1}$ .

Convert temperature to Kelvin.
$T_K = T_C + 273.15$ $T_K = 40^\circ\text{C} + 273.15 = 313.15 \text{ K}$
Use the ideal gas law, $PV = nRT$ , to calculate pressure $P$ .
$P = \frac{nRT}{V}$
Substitute the given values and calculate $P$ .
$P = \frac{(1 \text{ mol})(8.314 \text{ J} \cdot \text{mol}^{-1} \cdot \text{K}^{-1})(313.15 \text{ K})}{0.382 \times 10^{-3} \text{ m}^3}$ $P = \frac{2603.961 \text{ J}}{0.000382 \text{ m}^3}$
Since $1 \text{ J} = 1 \text{ N} \cdot \text{m}$ , then $\frac{J}{m^3} = \frac{N \cdot m}{m^3} = \frac{N}{m^2}

One mole of CO2(g) occupies 0.382 × 10−3 m³ at 40°C. Calculate the pressure that the gas would exert assuming ideal behavior. Take R = 8.314 J·mol⁻¹·K⁻¹.

Step-by-step solution

Convert temperature to Kelvin.

Use the ideal gas law, $PV = nRT$ , to calculate pressure $P$ .

Substitute the given values and calculate $P$ .

Still stuck on this one?

More Physics Questions

One mole of CO2(g) occupies 0.382 × 10−3 m³ at 40°C. Calculate the pressure that the gas would exert assuming ideal behavior. Take R = 8.314 J·mol⁻¹·K⁻¹.

Step-by-step solution

Convert temperature to Kelvin.

Use the ideal gas law, PV=nRTPV = nRTPV=nRT, to calculate pressure PPP.

Substitute the given values and calculate PPP.

Still stuck on this one?

More Physics Questions

Use the ideal gas law, $PV = nRT$ , to calculate pressure $P$ .

Substitute the given values and calculate $P$ .