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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.

Respuesta :

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

Answer:

8.935 × 10⁴ kJ

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:

[tex]5743gC_{6}H_{12}O_{6}.\frac{1molC_{6}H_{12}O_{6}}{180.16gC_{6}H_{12}O_{6}} .\frac{2803kJ}{1molC_{6}H_{12}O_{6}} = 8.935 \times 10^{4} kJ[/tex]

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