A 27.8 liter container is initially evacuated, and then 8.8 grams of water is placed in it. After a time, all the water evaporates, and the temperature is 130.8 degrees C. Find the final pressure.
PV=nRT
P= nRT/V all you have to do is convert 8 grams water to moles water. tEmps in Kelvin
Ok thanks, so do you just find the molar mass of those 8 grams of water to find moles?
To find the final pressure in the container, we can use the Ideal Gas Law equation, which states:
PV = nRT
Where:
P - pressure
V - volume of the container
n - number of moles of the gas
R - ideal gas constant
T - temperature in Kelvin
First, we need to convert the given temperature from degrees Celsius to Kelvin. The temperature in Kelvin can be calculated by adding 273.15 to the Celsius temperature:
T (Kelvin) = 130.8 + 273.15 = 404.95 K
The next step is to calculate the number of moles of water that evaporated. To do this, we need to convert the mass of water given (8.8 grams) to moles using the molar mass of water (18.015 g/mol):
moles of water = mass of water / molar mass of water
= 8.8 g / 18.015 g/mol
= 0.4887 mol
Now we can substitute the values into the Ideal Gas Law equation:
PV = nRT
P * 27.8 L = 0.4887 mol * 0.0821 L·atm/mol·K * 404.95 K
Simplifying the equation:
P = (0.4887 mol * 0.0821 L·atm/mol·K * 404.95 K) / 27.8 L
Calculating this expression will give us the final pressure in atmospheres.