5. Gas in a constant-volume gas thermometer registers a pressure of $95.0 \mathrm{kPa}$ at $100^{\circ} \mathrm{C}$. Assuming ideal behavior, what is the temperature of this gas when the pressure is $190 \mathrm{kPa}$ ?
a) $546^{\circ} \mathrm{C}$
b) $527^{\circ} \mathrm{C}$
c) $491^{\circ} \mathrm{C}$
d) $473^{\circ} \mathrm{C}$

Step 1 ：Given that the initial pressure \(P_1\) is 95.0 kPa and the initial temperature \(T_1\) is 100°C, we are asked to find the final temperature \(T_2\) when the pressure is doubled to 190 kPa.

Step 2 ：First, we need to convert the initial temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is \(K = °C + 273.15\). So, \(T_1 = 100°C + 273.15 = 373.15 K\).

Step 3 ：Since the volume is constant and the gas is ideal, we can use the ideal gas law which states that the pressure of a gas is directly proportional to its temperature (in Kelvin), if the volume and the amount of gas are kept constant. This means that if the pressure is doubled, the temperature (in Kelvin) should also be doubled. So, \(T_2 = 2 \times T_1 = 2 \times 373.15 K = 746.3 K\).

Step 4 ：Finally, we need to convert the final temperature from Kelvin back to Celsius. The formula to convert Kelvin to Celsius is \(°C = K - 273.15\). So, \(T_2 = 746.3 K - 273.15 = 473.15°C\).

Step 5 ：Final Answer: The temperature of the gas when the pressure is \(190 kPa\) is \(\boxed{473°C}\). Therefore, the correct answer is (d) \(473°C\).