What gas volume does the water have at a temperature of 100 and 1 pressure?
What gas volume does the water liquid or gas or solid? have at a temperature of 100 what and 1 what pressure?
For gasses I believe the equation is PV=nRT
n is the # of moles of the substance,
R is 8.13 (?) a constant,
T is the temperature in Kelvin,
V is the volume the gas occupies,
and P is the pressure.
To determine the gas volume of water at a specific temperature and pressure, we need to refer to the Ideal Gas Law equation. The equation is defined as follows:
PV = nRT
where:
- P represents pressure
- V represents volume
- n represents the number of moles of the gas
- R is the ideal gas constant
- T represents temperature in Kelvin
To use this equation, we need to convert the given temperature of 100°C to Kelvin. The Kelvin scale is an absolute temperature scale that starts at 0 Kelvin (-273.15°C). To convert Celsius to Kelvin, we add 273.15 to the given value:
T(K) = T(°C) + 273.15
So, T = 100°C + 273.15 = 373.15K
Now, let's assume that we are dealing with water vapor, which is H2O(g). The number of moles (n) is not given in the question. However, we can calculate the number of moles using the concept of molar mass.
The molar mass of water, H2O, is approximately:
- 2(1.0078 g/mol) + 15.9994 g/mol = 18.015 g/mol
Assuming we have one mole of water (n = 1), we can substitute the values into the Ideal Gas Law equation:
PV = nRT
(1)(V) = (1)(0.0821 L·atm/(K·mol))(373.15K)
At standard temperature and pressure (STP), 1 atm pressure is equal to 22.4 liters of volume for an ideal gas. Therefore, we can rearrange the equation as follows:
V = (0.0821 L·atm/(K·mol))(373.15K) / (1 atm)
Simplifying the equation, we get:
V = 30.11 L
Hence, the gas volume of one mole of water at a temperature of 100°C and 1 atm pressure is approximately 30.11 liters.