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)

The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 0 ° C

The correct answer is (A) : The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 0 C.