To solve this problem, we can use the ideal gas law, which states:
PV = nRT
Where: P = Pressure of the gas (constant) V = Volume of the gas n = Number of moles of the gas (constant for a given amount of gas) R = Ideal gas constant T = Temperature of the gas
Since the pressure is kept constant, we can rewrite the equation as:
V1/T1 = V2/T2
Where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.
Given: V1 = 250 cm³ T1 = 10 °C (Convert to Kelvin by adding 273.15: 10 + 273.15 = 283.15 K) V2 = 150 cm³
We can rearrange the equation to solve for T2:
T2 = (V2 * T1) / V1
Substituting the values:
T2 = (150 * 283.15) / 250 T2 = 169.98 K
Converting back to Celsius:
T2 = 169.98 - 273.15 ≈ -103.17 °C
Therefore, at a constant pressure, we would expect the temperature to be approximately -103.17 °C for the volume to be 150 cm³.