determine the mass of CO2 produced when 76.8g of CaO is reacted with 50.0 g of C acording to the unbalanced equation...
CaO + C ==> CaC2 CO2
after i balanced the equation i got
2CaO +5C ==> 2CaC2 +CO2
This is a limiting reagent problem. I know that when I see that BOTH reactants are given. I work these problems by solving two simple stoichiometry problems (simple meaning they are not limiting reagent problems.).
First you calculate the moles CO2 produced from the CaO. Second you determine the moles of CO2 produced from the C. In limiting reagent problems, the moles of product will be different and the correct answer is ALWAYS the smaller value. The reagent producing that value is the limiting reagent. Here is a link to solving simple stoichiometry problems.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the mass of CO2 produced, you can use stoichiometry.
Step 1: Convert the given masses of CaO and C to moles.
- Moles of CaO = mass of CaO / molar mass of CaO
Moles of CaO = 76.8 g / 56.08 g/mol (molar mass of CaO)
- Moles of C = mass of C / molar mass of C
Moles of C = 50.0 g / 12.01 g/mol (molar mass of C)
Step 2: Determine the stoichiometric ratio between CaO and CO2.
From the balanced equation: 2CaO + 5C → 2CaC2 + CO2
The stoichiometric ratio between CaO and CO2 is 2:1. This means that 2 moles of CaO produce 1 mole of CO2.
Step 3: Calculate the moles of CO2 produced.
Since we know the moles of CaO, we can use the stoichiometric ratio to determine the moles of CO2 produced.
Moles of CO2 = (moles of CaO) / 2
Step 4: Convert moles of CO2 to grams.
Mass of CO2 = Moles of CO2 * molar mass of CO2
Molar mass of CO2 = 44.01 g/mol
Now you can follow these steps using the given values to calculate the mass of CO2 produced.
To determine the mass of CO2 produced, we need to use stoichiometry, which involves balancing the equation and using the molar ratios.
Given:
Mass of CaO = 76.8 g
Mass of C = 50.0 g
Balanced equation:
2CaO + 5C → 2CaC2 + CO2
First, we need to convert the masses of CaO and C into moles. To do this, we can use the molar mass of each compound.
Molar mass of CaO:
Ca = 40.08 g/mol
O = 16.00 g/mol
Total = 40.08 + 16.00 = 56.08 g/mol
Moles of CaO = mass / molar mass = 76.8 g / 56.08 g/mol ≈ 1.37 mol
Molar mass of C = 12.01 g/mol
Moles of C = mass / molar mass = 50.0 g / 12.01 g/mol ≈ 4.16 mol
From the balanced equation, the ratio of moles of CaO to CO2 is 2:1. This means that 2 moles of CaO will produce 1 mole of CO2.
Using this ratio, we can determine the moles of CO2 produced:
Moles of CO2 = 1.37 mol CaO * (1 mol CO2 / 2 mol CaO) = 0.685 mol CO2
Finally, we convert the moles of CO2 into grams using its molar mass.
Molar mass of CO2:
C = 12.01 g/mol
O = 16.00 g/mol (x2)
Total = 12.01 + 16.00 + 16.00 = 44.01 g/mol
Mass of CO2 = moles * molar mass = 0.685 mol * 44.01 g/mol ≈ 30.16 g
Therefore, the mass of CO2 produced when 76.8 g of CaO is reacted with 50.0 g of C is approximately 30.16 grams.