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

April 6, 2026Physics

ScanSolve AI Answer

April 6, 2026

Answer

8.314 J \cdot mol^{-1} \cdot K^{-1}$.

Here are the solutions to your exercises:

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

Step 1: Convert temperature to Kelvin. $T_K = T_C + 273.15$

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1) One mole of CO_2(g) occupies 0.382 × 10^-3 m^3 at 40^. Calculate the pressure that the gas would exert assuming ideal behavior.

Asked on April 6, 2026Physics

This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.

ScanSolve AI AnswerAnswered on April 6, 2026

Here are the solutions to your exercises: 1) One mole of CO_2(g) occupies 0.382 × 10^-3 m^3 at 40^. Calculate the pressure that the gas would exert assuming ideal behavior. Take R = 8.314 J · mol^-1 · K^-1. Step 1: Convert temperature to Kelvin. T_K = T_C + 273.15 T_K = 40^ + 273.15 = 313.15 \