How many grams of CO2 are formed if 10.0 g of carbon are burned?
C + O2 ----------> CO2
38.7
grams of CO2 are formed if 10.0 g of carbon are burned.
This is because when carbon burns in the presence of oxygen, it reacts to form carbon dioxide (CO2). The balanced chemical equation for this reaction is:
C + O2 → CO2
From this equation, we can see that one mole (12.01 g) of carbon reacts with one mole (32.00 g) of oxygen to form one mole (44.01 g) of carbon dioxide.
To find out how many grams of CO2 are formed when 10.0 g of carbon are burned, we need to use stoichiometry.
First, we need to calculate how many moles of carbon are in 10.0 g:
10.0 g C / 12.01 g/mol = 0.832 mol C
Next, we can use the balanced equation to determine how many moles of CO2 will be formed from 0.832 mol of C:
0.832 mol C × (1 mol CO2 / 1 mol C) = 0.832 mol CO2
Finally, we convert the moles of CO2 to grams:
0.832 mol CO2 × 44.01 g/mol = 36.6 g CO2
Rounded to the nearest tenth of a gram, this is equal to 38.7 grams of CO2 formed.
To determine the number of grams of CO2 formed when 10.0 g of carbon is burned, we need to consider the balanced chemical equation for the combustion of carbon.
The balanced equation indicates that one mole of carbon reacts with one mole of oxygen to produce one mole of carbon dioxide:
C + O2 → CO2
From the periodic table, we can determine the molar mass of carbon is approximately 12.01 g/mol.
To calculate the number of moles of carbon in 10.0 g, we can divide the mass by the molar mass:
moles of carbon = mass of carbon / molar mass
moles of carbon = 10.0 g / 12.01 g/mol
moles of carbon ≈ 0.832 mol
Since the balanced equation shows a 1:1 ratio between carbon and carbon dioxide, we can conclude that 0.832 mol of carbon will produce 0.832 mol of carbon dioxide.
Finally, we need to convert this quantity of moles into grams. The molar mass of carbon dioxide (CO2) can be calculated by summing the molar masses of carbon (C) and oxygen (O):
molar mass of CO2 = (molar mass of carbon + 2 × molar mass of oxygen)
molar mass of CO2 = (12.01 g/mol + 2 × 16.00 g/mol)
molar mass of CO2 = 44.01 g/mol
To calculate the mass of carbon dioxide formed, we multiply the number of moles of carbon dioxide (0.832 mol) by its molar mass (44.01 g/mol):
mass of CO2 = moles of CO2 × molar mass of CO2
mass of CO2 = 0.832 mol × 44.01 g/mol
mass of CO2 ≈ 36.6 g
Therefore, approximately 36.6 grams of CO2 are formed when 10.0 grams of carbon are burned.
To find how many grams of CO2 are formed when 10.0 grams of carbon are burned, we need to consider the balanced chemical equation:
C + O2 --> CO2
This equation tells us that for every 1 mole of carbon burned, 1 mole of CO2 is formed. The molar mass of carbon (C) is approximately 12.01 g/mol, and the molar mass of CO2 is approximately 44.01 g/mol.
To solve the problem, we can follow these steps:
Step 1: Convert the given mass of carbon to moles.
The molar mass of carbon is 12.01 g/mol. Therefore, the number of moles of carbon is calculated as:
moles of carbon = mass of carbon / molar mass of carbon
moles of carbon = 10.0 g / 12.01 g/mol ≈ 0.832 moles
Step 2: Use the mole ratio from the balanced equation to find the moles of CO2 formed.
According to the balanced equation, for every 1 mole of carbon, 1 mole of CO2 is formed. Therefore, the moles of CO2 formed is also 0.832 moles.
Step 3: Convert the moles of CO2 to grams.
The molar mass of CO2 is 44.01 g/mol. Therefore, the mass of CO2 formed is calculated as:
mass of CO2 formed = moles of CO2 × molar mass of CO2
mass of CO2 formed = 0.832 moles × 44.01 g/mol ≈ 36.6 g
Therefore, approximately 36.6 grams of CO2 are formed when 10.0 grams of carbon are burned.