A sample of 10.7 g of O2 reacts completely with CO to form CO2.
2 CO + O2 → 2 CO2. How many grams of CO is required.
To find the number of grams of CO required, we need to use stoichiometry and the given amount of O2.
1. Start by figuring out the molar mass of O2 (oxygen gas). The molar mass of oxygen is approximately 32.00 g/mol.
2. Next, calculate the number of moles of O2 in the given sample. Divide the mass of O2 (10.7 g) by its molar mass.
moles of O2 = mass of O2 / molar mass of O2
= 10.7 g / 32.00 g/mol
= 0.334 mol
3. Now, let's use the balanced chemical equation to determine the mole ratio between O2 and CO.
According to the balanced equation: 2 CO + O2 → 2 CO2, the ratio is 2:1.
This means that for every 1 mole of O2, 2 moles of CO are needed.
4. Multiply the number of moles of O2 by the mole ratio to find the number of moles of CO.
moles of CO = moles of O2 × (2 moles of CO / 1 mole of O2)
= 0.334 mol × 2
= 0.668 mol
5. Finally, determine the mass of CO by multiplying the number of moles by its molar mass.
mass of CO = moles of CO × molar mass of CO
= 0.668 mol × (molar mass of CO)
To calculate the molar mass of CO, we need to know the individual molar masses of carbon and oxygen. Since it is not provided, we cannot determine the exact mass of CO without this information.
This reaction requires twice the moles of CO as O2.
MolesO2=10.7/32
molesCO=2x above
gramsCO=2*10.7/32*molmassCO
and the mole mass of CO is 28