Question

how many grams of CO2 are required in order to produce 120.0 g of glucose

Answer 1

Answer:

6 grams of $CO_2$ are required to produce 120 g of glucose

Explanation:

if you multiply 6 * 2 from the equation $6CO_2$ you get 120 as the answer

HOPE SO IT'S CORRECT

Answer 2

Answer:

There will be 175.9 g of CO2 in 120.0 g of glucose.

Explanation:

Answer:

There are 4 steps to do this stoichiometry question.

1. Find the balanced chemical equation of glucose which is,

      6CO2   +   6H2O   ----->   C6H12O6   +   6O2

2. Convert the mass (g) of glucose in moles.

3. Solve for the moles of CO" using the mole-mole ratio.

4. Now we all get what we need, we can solve for the mass of CO2 using the formula m=nM ( m stands for mass, n stands for # of moles and, M for molar mass).

Given: 120 g of glucose (C6H12O6)

            6CO2   +   6H2O   ----->   C6H12O6   +   6O2

Find: mass of CO2

Solution: The mass of glucose ---> moles (n).

Molar mass of glucose=  12.011(6) + 1.0097(12) + 15.999 (6)

                                    =  180.155 g/mol

- So now we have the mass of glucose which is 120, and Molar mass which is 180.155 g/mol... we can use the formula n = m/M to get the moles.

n=m/M

n= 120 g/ 180.155 g/mol

= 0.666 mol of glucose

Now let's find the moles of CO2 using the mole-mole ratio. (note: we get that 6 and 1 in the numerical number of the balanced equation.) Use cross multiplication.

      x mole of CO2/ 6  =   0.666 mol of glucose/1

        x = 3.996 mol of CO2

Now we have the mole of CO2, it's easy to find it's molar mass and mass in grams.

Molar mass of CO2 = 12.011 + 15.999(2)

                                = 44.01 g/mol

m=nM

mass of CO2 = 3.996 mol x 44.01 g/mol

mass of CO2 = 175.86 or roughly 175.9 g

Therefore, the mass of CO2 that can be produced is 175.9 g.