To solve this problem, we can use the combined gas law, which relates the initial and final conditions of pressure, volume, and temperature for a gas sample. The combined gas law equation is as follows:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where: P1 = Initial pressure V1 = Initial volume T1 = Initial temperature P2 = Final pressure V2 = Final volume T2 = Final temperature
Let's plug in the given values into the equation:
P1 = 660.0 torr V1 = 280.0 mL T1 = 26.0°C + 273.15 (converting to Kelvin) = 299.15 K P2 = 940.0 torr V2 = 440.0 mL
Now we can solve for T2:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
(T2) = (P2 * V2 * T1) / (P1 * V1)
(T2) = (940.0 torr * 440.0 mL * 299.15 K) / (660.0 torr * 280.0 mL)
Calculating this expression:
(T2) ≈ 391.47 K
Therefore, the temperature at which the neon sample would exert a pressure of 940 torr in a volume of 440 mL, assuming the number of moles remains constant, is approximately 391.47 Kelvin.