Two gas samples have the same number of molecules, the same volume, and the same pressure. Which of the following could be true?
A. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 0o C. B. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 298 K. C. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 273o C. D. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 100o C.
Lets name one gas sample as A and other gas sample as B. we can apply ideal gas law equation for both samples PV = nRT P - Pressure of A = Pressure of B V - volume of A = volume of B n - number of molecules of both A and B being equal is equivalent to number of moles of A = number of moles of B R - universal gas constant Tᵃ - temperature of A Tᵇ - temperature of B for gas A PV = nRTᵃ --1) for gas B PV = nRTᵇ ---2) when we divide both equations 1 = Tᵃ / Tᵇ Tᵃ = Tᵇ both temperatures are equal temperature in Celsius + 273 = temperature in Kelvin therefore 0 °C = 273 K the correct answer is A) <span>The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 0 </span>°<span>C</span>
