In photosynthesis, glucose, C6H12O6, and O2 are produced from CO2 and H2O. Glucose from starches is the major fuel for the body.
6CO2(g)+6H2O(l)+680kcal⟶ C6H12O6(aq)+6O2(g)
How much heat, in kilojoules, is needed to produce 22.5 g of C6H12O6?
for anyone looking for the answers to Cell Work and Carbon Quick Check it is
1. CO2+H2O
2. 36
3. There are no chloroplasts in the plants cells
4. both processes involve carbon compounds…
5. Oxygen from the atmosphere reacts with glucose
To calculate the amount of heat required to produce 22.5 g of C6H12O6, we will first determine the amount of moles of C6H12O6 produced and then use the given enthalpy change to calculate the heat.
Step 1: Calculate the amount of moles of C6H12O6 produced.
The molar mass of C6H12O6 is:
(6 × atomic mass of C) + (12 × atomic mass of H) + (6 × atomic mass of O)
= (6 × 12.01 g/mol) + (12 × 1.01 g/mol) + (6 × 16.00 g/mol)
= 72.06 g/mol
Given that the mass of C6H12O6 produced is 22.5 g, we can calculate the number of moles using the formula:
moles = mass / molar mass
= 22.5 g / 72.06 g/mol
= 0.312 mol
Step 2: Convert the given enthalpy change to kJ/mol.
The given enthalpy change is 680 kcal. We need to convert kcal to kJ. There are 4.184 kJ in 1 kcal, so:
680 kcal = 680 × 4.184 kJ
= 2840.72 kJ
Step 3: Calculate the heat required.
Now that we know the number of moles produced and the enthalpy change per mole, we can calculate the heat required using the formula:
heat = moles × enthalpy change
= 0.312 mol × 2840.72 kJ/mol
= 886.9 kJ
Therefore, the amount of heat, in kilojoules, needed to produce 22.5 g of C6H12O6 is approximately 886.9 kJ.