the following reaction consumes 2.6kg of CO(g): CO(g) + H2O(g) --> CO2(g) + H2(g)
how many total liters of gas are formed if the products are collected at STP?
To find the total volume of gas formed at STP (Standard Temperature and Pressure), you first need to calculate the number of moles of CO2 and H2 produced.
1. Calculate the number of moles of CO2:
The molar mass of CO2 is 44.01 g/mol.
Given that 2.6 kg of CO is consumed, you need to convert it to moles:
Moles of CO2 = mass of CO2 / molar mass of CO2
Moles of CO2 = (2.6 kg / 44.01 g/mol)
2. Calculate the number of moles of H2:
The molar mass of H2 is 2.02 g/mol.
Since the balanced chemical equation shows a 1:1 stoichiometric ratio between CO2 and H2, the number of moles of H2 will be the same as CO2.
3. Calculate the total volume of gas at STP:
At STP, 1 mole of any ideal gas occupies 22.4 liters of volume.
Thus, the total volume of gas formed will be:
Volume of gas = Total moles of gas × 22.4 L/mol
For this case, Volume of gas = (Moles of CO2 + Moles of H2) × 22.4 L/mol
Now you can substitute the values into the equation to find the total volume of gas formed.