When 6.000 moles of glucose are combusted, 16815 kJ of energy is produ

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When 6.000 moles of glucose are combusted, 16815 kJ of energy is produced. Which of the following chemical equations represent this process? 6C6H12O6(s) + 36O2(g) → 36CO2(g) + 36H2O(l) ΔH = −2802.5 kJ 6C6H12O6(s) + 36O2(g) → 36CO2(g) + 36H2O(l) ΔH = 16815 kJ C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH = −16815 kJ C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH = −2802.5 kJ all equations are correct

When 6.000 moles of glucose are combusted, 16815 kJ of energy is produced. Which of the following chemical equations represent this process? 6C6H12O6(s) + 36O2(g) → 36CO2(g) + 36H2O(l) ΔH = −2802.5 kJ 6C6H12O6(s) + 36O2(g) → 36CO2(g) + 36H2O(l) ΔH = 16815 kJ C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH = −16815 kJ C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH = −2802.5 kJ all equations are correct

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When 6.000 moles of glucose are combusted,

16815 k J

of energy is produced. Which of the following chemical equations represent this process?

6 C 6 H 12 O 6 (s) + 36 O 2 (g) \to 36 C O 2 (g) + 36 H 2 O (l)

Δ H = - 2802.5 k J

6 C 6 H 12 O 6 (s) + 36 O 2 (g) \to 36 C O 2 (g) + 36 H 2 O (l)

Δ H = 16815 k J

C 6 H 12 O 6 (s) + 6 O 2 (g) \to 6 C O 2 (g) + 6 H 2 O (l)

Δ H = - 16815 k J

C 6 H 12 O 6 (s) + 6 O 2 (g) \to 6 C O 2 (g) + 6 H 2 O (l)

Δ H = - 2802.5 k J

all equations are correct

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