Question

Given the thermochemical equation for photosynthesis, 6h2o(l) + 6co2(g) → c6h12o6(s) + 6o2(g) δh = +2803 kj/mol calculate the solar energy required to produce 5743 g of c6h12o6.

Answer 1

2832 g glucose x 1 mol/180 g = 15.73 moles glucose
2803 kJ/mole x 15.73 moles = 44,100 kJ

Answer 2

8.935 × 10⁴ kJ

Step-by-step explanation:

Let's consider the thermochemical equation for photosynthesis.

6 H₂O(l) + 6 CO₂(g) → C₆H₁₂O₆(s) + 6 O₂(g) ΔH = +2803 kJ/mol

2803 kJ of energy are absorbed per 1 mole of C₆H₁₂O₆. Considering the molar mass of C₆H₁₂O₆ is 180.16 g/mol, the energy required to produce 5743 g of C₆H₁₂O₆ is:

`5743gC_(6)H_(12)O_(6).(1molC_(6)H_(12)O_(6))/(180.16gC_(6)H_(12)O_(6)) .(2803kJ)/(1molC_(6)H_(12)O_(6)) = 8.935 * 10^(4) kJ`