How many grams of CO2 is produced from 855 grams of C6H12O6 in the process of cell respiration?

To determine the number of grams of CO2 produced from 855 grams of C6H12O6, we need to consider the balanced equation for the process of cell respiration. The equation is as follows:

C6H12O6 + 6O2 → 6CO2 + 6H2O

According to the equation, one molecule of C6H12O6 produces 6 molecules of CO2. To calculate the grams of CO2 produced, we can follow these steps:

1. Determine the molar mass of C6H12O6:
C6H12O6 = (6 * atomic mass of carbon) + (12 * atomic mass of hydrogen) + (6 * atomic mass of oxygen)

By looking up the atomic mass values, we can calculate the molar mass of C6H12O6.

2. Convert grams of C6H12O6 to moles:
Moles of C6H12O6 = grams of C6H12O6 / molar mass of C6H12O6

Divide the given 855 grams of C6H12O6 by the calculated molar mass from step 1.

3. Determine the moles of CO2 produced:
Moles of CO2 = Moles of C6H12O6 * (6 moles of CO2 / 1 mole of C6H12O6)

Multiply the moles of C6H12O6 (from step 2) by the ratio of moles of CO2 to moles of C6H12O6.

4. Convert moles of CO2 to grams:
Grams of CO2 = Moles of CO2 * molar mass of CO2

Multiply the moles of CO2 (from step 3) by the molar mass of CO2 to get the final answer in grams.

By following these steps, you can determine the number of grams of CO2 produced from 855 grams of C6H12O6 in the process of cell respiration.