How many grams of CO are produced when 40.0 g of C reacts?
To calculate the number of grams of CO produced when 40.0 g of C reacts, we need to use the balanced chemical equation for the reaction between C (carbon) and O2 (oxygen) to form CO (carbon monoxide):
C + O2 -> CO
According to the equation, for every 1 mole of C that reacts, 1 mole of CO is produced. The molar mass of C is 12.01 g/mol, and the molar mass of CO is 28.01 g/mol.
First, we need to determine the number of moles of C in 40.0 g:
moles of C = mass of C / molar mass of C
moles of C = 40.0 g / 12.01 g/mol
moles of C = 3.33 mol (approx.)
Since the balanced chemical equation states that the ratio of C to CO is 1:1, the number of moles of CO produced will also be 3.33 mol.
Finally, we can calculate the mass of CO produced by multiplying the number of moles of CO by the molar mass of CO:
mass of CO = moles of CO * molar mass of CO
mass of CO = 3.33 mol * 28.01 g/mol
mass of CO = 93.23 g (approx.)
Therefore, when 40.0 g of C reacts, approximately 93.23 grams of CO are produced.
To determine the number of grams of CO (carbon monoxide) produced when 40.0 g of C (carbon) reacts, we need to use the balanced chemical equation for the reaction between carbon and oxygen.
The balanced chemical equation for the formation of carbon monoxide is:
C + O2 -> CO
According to the equation, 1 mole of carbon reacts with 1 mole of oxygen to produce 1 mole of carbon monoxide.
To calculate the number of moles of carbon in 40.0 g, we need to divide the mass of carbon by its molar mass. The molar mass of carbon is 12.01 g/mol.
Moles of carbon = mass of carbon / molar mass of carbon
Moles of carbon = 40.0 g / 12.01 g/mol
Moles of carbon = 3.33 mol (approximately)
Since the reaction is 1:1, the number of moles of carbon monoxide produced will also be 3.33 mol.
Now, to calculate the mass of carbon monoxide produced, we multiply the number of moles of carbon monoxide by its molar mass. The molar mass of carbon monoxide is 28.01 g/mol.
Mass of carbon monoxide = moles of carbon monoxide x molar mass of carbon monoxide
Mass of carbon monoxide = 3.33 mol x 28.01 g/mol
Mass of carbon monoxide = 93.0933 g (approximately)
Therefore, approximately 93.09 grams of carbon monoxide (CO) are produced when 40.0 grams of carbon (C) reacts.
To determine the number of grams of CO produced when 40.0 g of C reacts, we need to use the stoichiometry of the balanced chemical equation that describes the reaction. The balanced equation tells us the ratio of moles between the reactants and products. Here is the balanced equation for the reaction of C (carbon) with O2 (oxygen) to form CO (carbon monoxide):
C + O2 → CO
To calculate the number of grams of CO produced, follow these steps:
Step 1: Convert the mass of C to moles
To convert grams to moles, we need to divide the given mass by the molar mass of carbon (C), which is approximately 12.01 g/mol.
40.0 g C × (1 mol C / 12.01 g C) = 3.33 mol C
Step 2: Apply stoichiometry
Using the balanced equation, we can see that the ratio between C and CO is 1:1. This means that for every 1 mole of carbon (C), we obtain 1 mole of carbon monoxide (CO).
Since we have 3.33 moles of carbon, we would also have 3.33 moles of carbon monoxide.
Step 3: Convert moles of CO to grams
To convert moles of CO to grams, we need to multiply the number of moles by the molar mass of carbon monoxide (CO), which is approximately 28.01 g/mol.
3.33 mol CO × (28.01 g CO / 1 mol CO) = 93.0 g CO
Therefore, when 40.0 g of carbon reacts, approximately 93.0 grams of carbon monoxide are produced.