un gaz parfait occupe un cylindre de 5.0×10² ml de volume ; la température est de 30.0 °c et la pression de…

Explanation:

Step1: Convert temperatures to Kelvin

The initial temperature $T_1 = 30.0^{\circ}C+273.15 = 303.15$ K. The final temperature $T_2=520^{\circ}C + 273.15=793.15$ K. The initial volume $V_1 = 5.0\times10^{2}$ mL and the final volume $V_2 = 25.0$ mL. The initial pressure $P_1=95.0$ kPa.

Step2: Use the combined - gas law formula

The combined - gas law is $\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$. We want to find $P_2$. Rearranging the formula for $P_2$ gives $P_2=\frac{P_1V_1T_2}{V_2T_1}$.

Step3: Substitute the values

$P_2=\frac{95.0\text{ kPa}\times5.0\times 10^{2}\text{ mL}\times793.15\text{ K}}{25.0\text{ mL}\times303.15\text{ K}}$ $P_2=\frac{95.0\times5.0\times10^{2}\times793.15}{25.0\times303.15}\text{ kPa}$ $P_2=\frac{95.0\times5.0\times793.15}{25.0\times3.0315}\text{ kPa}$ $P_2=\frac{95.0\times5.0\times793.15}{75.7875}\text{ kPa}$ $P_2 = 5000$ kPa

Answer:

5000 kPa