A gas has a pressure of 710 kPa at 227 Celsius. What will its pressure be at 27 Celsius, if the volume does not change?
Idk
To solve this question, we can use the ideal gas law, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature in Kelvin
First, let's convert the temperatures from Celsius to Kelvin. The Kelvin temperature is obtained by adding 273.15 to the Celsius temperature.
Given:
P1 = 710 kPa
T1 = 227 °C
T2 = 27 °C
Converting the temperatures to Kelvin:
T1 = 227 + 273.15 = 500.15 K
T2 = 27 + 273.15 = 300.15 K
Since the volume does not change, we can assume that V1 = V2.
Using the ideal gas law equation, we can set up the following equation:
P1V1 = P2V2
Since V1 = V2, we can simplify the equation to:
P1 = P2
Therefore, the pressure of the gas at 27 °C will be the same as its initial pressure, which is 710 kPa.
(P1/T1) = (P2/T2)
T must be in kelvin.