Final answer:
The new pressure of the helium gas is 112.65 kPa when the temperature is raised to 333 K.
Step-by-step explanation:
According to Charles's Law, the volume of a gas is directly proportional to its temperature when pressure is constant. Using this law, we can find the new pressure of the helium gas.
First, we need to convert the temperatures to Kelvin by adding 273 to the given values. The initial temperature is 303 K and the final temperature is 333 K.
Using the equation V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature, we can calculate the new volume of the gas.
Since the volume is constant, V1 = V2. Plugging in the values, we have (V1/303) = (V1/333). Solving for V1, we get V1 = V2 * (T1/T2).
Now we can substitute the initial pressure of 102 kPa and the calculated volume of 0.300 L into the ideal gas law equation PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. Rearranging the equation, we get P = (nRT)/V.
Given that R is a constant, the number of moles remains constant, and the volume is constant, we can simplify the equation P1 = P2 * (T1/T2), where P1 is the initial pressure and P2 is the final pressure. Plugging in the values, we find P2 = P1 * (T2/T1).
Substituting the values, P2 = (102 kPa) * (333 K / 303 K) = 112.65 kPa.