What is the molar volume of H2 at 1.50 atm and -25 degrees celcius?
To find the molar volume of H2 at a given pressure and temperature, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, let's convert the given temperature from Celsius to Kelvin. To do this, we add 273.15 to the Celsius temperature. So -25 degrees Celsius is equal to -25 + 273.15 = 248.15 Kelvin.
Next, we need to find the number of moles of H2. This information is not provided in the question, so we'll assume you are given the number of moles or that the sample is in standard conditions, where 1 mole of any ideal gas occupies 22.4 liters.
Now we can rearrange the ideal gas law equation to solve for the volume:
V = (nRT) / P
Plug in the values:
V = (n * 0.0821 * 248.15) / 1.50
Since we don't have the number of moles, we cannot calculate the exact molar volume in liters. However, if you have the number of moles of H2, you can substitute that value into the equation to find the molar volume.