Step 1: Convert temperatures from Celsius to Kelvin. To convert Celsius to Kelvin, add 273.15. $$T_1 = 27 \, ^\circ\text{C} + 273.15 = 300.15 \, \text{K}$$ $$T_2 = 20 \, ^\circ\text{C} + 273.15 = 293.15 \, \text{K}$$ Step 2: Identify the given values. Initial Volume ($V_1$) = $300 \, \text{cm}^3$ Initial Pressure ($P_1$) = $600 \, \text{kPa}$ Initial Temperature ($T_1$) = $300.15 \, \text{K}$ Final Volume ($V_2$) = $200 \, \text{cm}^3$ Final Temperature ($T_2$) = $293.15 \, \text{K}$ Final Pressure ($P_2$) = ? Step 3: Apply the Combined Gas Law. The Combined Gas Law states that for a fixed amount of gas, the ratio of the product of pressure and volume to the absolute temperature is constant: $$\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$$ To find $P_2$, rearrange the formula: $$P_2 = \frac{P_1 V_1 T_2}{T_1 V_2}$$ Step 4: Substitute the values and calculate $P_2$. $$P_2 = \frac{(600 \, \text{kPa}) \times (300 \, \text{cm}^3) \times (293.15 \, \text{K})}{(300.15 \, \text{K}) \times (200 \, \text{cm}^3)}$$ $$P_2 = \frac{52767000 \, \text{kPa} \cdot \text{cm}^3 \cdot \text{K}}{60030 \, \text{K} \cdot \text{cm}^3}$$ $$P_2 \approx 878.99 \, \text{kPa}$$ The pressure the gas would exert is approximately 879 kPa. 3 done, 2 left today. You're making progress.