What volume will 3.5g of CO occupy at 17 degrees Celsius and 1875 torr?
PV = nRT. Remember the units. Also T must be in kelvin.
To calculate the volume of a gas at a given temperature and pressure, you can use the Ideal Gas Law equation:
PV = nRT
Where:
P = Pressure (in units of force per unit area, such as torr or atm)
V = Volume (in units such as liters or milliliters)
n = Number of moles (in units of moles)
R = Ideal Gas Constant (varies depending on the units used for pressure and volume)
T = Temperature (in units of Kelvin)
In our case, we are given:
Pressure (P) = 1875 torr
Temperature (T) = 17 degrees Celsius
Before we can use the ideal gas law, we need to convert the given temperature from Celsius to Kelvin because the ideal gas law requires temperature to be in Kelvin. The Celsius to Kelvin conversion can be done by adding 273.15 to the Celsius temperature.
So, the Temperature (T) in Kelvin would be:
T(K) = 17 + 273.15
Now, we need to rearrange the ideal gas law equation to solve for volume (V):
V = (nRT) / P
Since we are given the mass of CO (3.5g), we can calculate the number of moles (n) using the formula:
n = mass / molar mass
The molar mass of carbon monoxide (CO) is 12.01 g/mol + 16.00 g/mol = 28.01 g/mol.
Now, we have enough information to calculate the number of moles (n). Let's substitute the values into the formulas:
n = 3.5g / 28.01 g/mol
After calculating the value of 'n', we can substitute it, along with the other given values, into the rearranged ideal gas law equation to find the volume:
V = (nRT) / P
Substitute the values and calculate the volume to get your answer.