Question

A 26.4 ml sample of ethylene gas C���H��� has a pressure of 2.50 atm at 2.5 degrees Celsius. If the volume is increased to 36.2 ml and the temperature is raised to 10 degrees Celsius, what is the new pressure?

Answer 1

To solve for the new pressure, we can use the combined gas law equation and plugging in the given values. By rearranging the equation, we can calculate the new pressure.

Step-by-step explanation:

To solve this problem, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

Plugging in the given values:

P1 = 2.50 atm
V1 = 26.4 ml = 0.0264 L
T1 = 2.5 °C + 273.15 = 275.65 K
V2 = 36.2 ml = 0.0362 L
T2 = 10 °C + 273.15 = 283.15 K

We can rearrange the equation to solve for the new pressure:

P2 = (P1 * V1 * T2) / (V2 * T1)

Substituting the values:

P2 = (2.50 atm * 0.0264 L * 283.15 K) / (0.0362 L * 275.65 K)

Simplifying the calculation will give us the new pressure.