Carbon monooxide CO is product of incomplete combustion of fuel. Find the volume that 42g of CO gas occupies at STP.
1 mole of any gas (28 g for CO) occupies a volume of 22.4 L at STP.
To find the volume of 42g of CO gas at STP (Standard Temperature and Pressure), we need to use the Ideal Gas Law equation, which is represented as:
PV = nRT
Where:
- P is the pressure (which is equal to 1 atm at STP)
- V is the volume
- n is the number of moles of gas
- R is the ideal gas constant (0.0821 L·atm/(mol·K))
- T is the temperature (which is equal to 273.15 K at STP)
To find the number of moles (n) of CO gas, we need to use the molar mass of CO, which is calculated by adding the atomic masses of carbon (C) and oxygen (O). The atomic mass of carbon is 12.01 g/mol, and the atomic mass of oxygen is 16.00 g/mol.
Molar mass of CO = (12.01 g/mol) + (16.00 g/mol) = 28.01 g/mol
Now we can calculate the number of moles (n) of CO gas:
n = molar mass / mass
n = 28.01 g/mol / 42 g
n = 0.667 mol
Now that we have the number of moles (n), we can rearrange the Ideal Gas Law equation to solve for the volume (V):
V = nRT / P
V = (0.667 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K) / (1 atm)
V ≈ 15.8 L
Therefore, 42g of CO gas occupies approximately 15.8 liters at STP.