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kykrilka [37]
3 years ago
9

What is the minimum amount of energy a plantmust absorb to produce 15.0 g of glucose?​

Chemistry
1 answer:
vekshin13 years ago
8 0

Answer:

The minimum amount of energy a plant  must absorb to produce 15.0 g of glucose is 57.0 kilo calories.

Explanation:

Energy released on combustion of 1 g gram of glucose = -3.80 kcal

Energy released on combustion of 1 grams of glucose = -3.80 kcal

So, the energy required to form 1 gram of glucose is = 3.80 kcal

The energy absorbed by the plants to produce 15 grams of glucose be :

15.0 g\times 3.8 kcal/g=57.0 kcal

The minimum amount of energy a plant  must absorb to produce 15.0 g of glucose is 57.0 kilo calories.

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Consider the following reaction:
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Answer:

1. d[H₂O₂]/dt = -6.6 × 10⁻³ mol·L⁻¹s⁻¹; d[H₂O]/dt = 6.6 × 10⁻³ mol·L⁻¹s⁻¹

2. 0.58 mol

Explanation:

1.Given ΔO₂/Δt…

    2H₂O₂     ⟶      2H₂O     +     O₂

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 d[H₂O]/dt =  2d[O₂]/dt =  2 × 3.3 × 10⁻³ mol·L⁻¹s⁻¹ =  6.6 × 10⁻³mol·L⁻¹s⁻¹

2. Moles of O₂  

(a) Initial moles of H₂O₂

\text{Moles} = \text{1.5 L} \times \dfrac{\text{1.0 mol}}{\text{1 L}} = \text{1.5 mol }

(b) Final moles of H₂O₂

The concentration of H₂O₂ has dropped to 0.22 mol·L⁻¹.

\text{Moles} = \text{1.5 L} \times \dfrac{\text{0.22 mol}}{\text{1 L}} = \text{0.33 mol }

(c) Moles of H₂O₂ reacted

Moles reacted = 1.5 mol - 0.33 mol = 1.17 mol

(d) Moles of O₂ formed

\text{Moles of O}_{2} = \text{1.33 mol H$_{2}$O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{2 mol H$_{2}$O}_{2}} = \textbf{0.58 mol O}_{2}\\\\\text{The amount of oxygen formed is $\large \boxed{\textbf{0.58 mol}}$}

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Where did the molecules of carbon dioxide come from while the tortilla chip was burning
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