A sample of hydrogen exerts a pressure of 0.418 atm at 57.0° C. The gas is heated to 88.0° C at constant volume. What will its new pressure be?
P2=P1*T2/T1 temps in Kelvins, please
To find the new pressure of the hydrogen gas, we can use the ideal gas law equation:
PV = nRT
where:
P is the pressure of the gas,
V is the volume of the gas,
n is the number of moles of gas,
R is the ideal gas constant, and
T is the temperature in Kelvin.
First, we need to convert the given temperatures from Celsius to Kelvin. The formula for converting Celsius to Kelvin is:
T(K) = T(°C) + 273.15
So, the initial temperature (T1) in Kelvin is:
T1 = 57.0°C + 273.15 = 330.15 K
And the final temperature (T2) in Kelvin is:
T2 = 88.0°C + 273.15 = 361.15 K
Since the volume of the gas is constant, V1 = V2. Therefore, we can write the equation as:
P1 * V1 = P2 * V2
where P1 is the initial pressure and P2 is the final pressure.
Now, rearranging the equation to solve for P2, we get:
P2 = (P1 * V1) / V2
We are given the initial pressure (P1) = 0.418 atm and the initial volume (V1) is not specified.
However, since the volume is constant, we can assume V1 = V2, and we can cancel out the V1 and V2 terms in the equation:
P2 = P1
So, the new pressure of the hydrogen gas after heating it to 88.0 °C at constant volume will be 0.418 atm.