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nika2105 [10]
3 years ago
11

The light reactions stage:

Chemistry
2 answers:
pychu [463]3 years ago
8 0

The light reactions stage occurs before the Calvin cycle , requires light energy to work  and releases oxygen through the stomata.

Answer: D) all the above

Explanation

The light reactions stage is one of the two stages which occur during the chemical reaction of photosynthesis.

It is the first stage and second stage is Calvin cycle. So the first option is true which states that the light reactions stage occurs before the Calvin cycle.

In light reactions stage, the light energy of sun is captured by the chloroplast and this energy is the main trigger for starting the light reaction stage between the reactants carbon-di-oxide and water.

So the second option is also true i.e., the light reactions require light energy to work.

In light reaction stage, the water molecules will release oxygen gas from the stomata.

Thus all the options are true for light reactions stage in photosynthesis.

hram777 [196]3 years ago
7 0

Answer:

(D) all of the above

Explanation:

The light reactions stage, occurs before the Calvin cycle, requires light energy to work, and releases oxygen through the stomata.

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Answer : The correct option is, (D) 3600 kJ

Explanation :

Mass of octane = 75 g

Molar mass of octane = 114.23 g/mole

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First we have to calculate the moles of octane.

\text{ Moles of octane}=\frac{\text{ Mass of octane}}{\text{ Molar mass of octane}}=\frac{75g}{114.23g/mole}=0.656moles

Now we have to calculate the heat released in the reaction.

As, 1 mole of octane released heat = -5500 kJ

So, 0.656 mole of octane released heat = 0.656 × (-5500 kJ)

                                                                   = -3608 kJ

                                                                   ≈ -3600 kJ

Therefore, the heat released in the reaction is 3600 kJ

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2 years ago
Great amounts of atomic energy are released when a _______reaction occurs.
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Which of the following will increase entropy in a reaction?
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Calculate the pH and fraction of dissociation ( α ) for each of the acetic acid ( CH 3 COOH , p K a = 4.756 ) solutions. A 0.002
marysya [2.9K]

Answer:

The degree of dissociation of acetic acid is 0.08448.

The pH of the solution is 3.72.

Explanation:

The pK_a=4.756

The value of the dissociation constant = K_a

pK_a=-\log[K_a]

K_a=10^{-4.756}=1.754\times 10^{-5}

Initial concentration of the acetic acid = [HAc] =c = 0.00225

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HAc\rightleftharpoons H^++Ac^-

Initially

c

At equilibrium ;

(c-cα)                                cα        cα

The expression of dissociation constant is given as:

K_a=\frac{[H^+][Ac^-]}{[HAc]}

1.754\times 10^{-5}=\frac{c\times \alpha \times c\times \alpha}{(c-c\alpha)}

1.754\times 10^{-5}=\frac{c\alpha ^2}{(1-\alpha)}

1.754\times 10^{-5}=\frac{0.00225 \alpha ^2}{(1-\alpha)}

Solving for α:

α = 0.08448

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[H^+]=c\alpha = 0.00225M\times 0.08448=0.0001901 M

The pH of the solution ;

pH=-\log[H^+]

=-\log[0.0001901 M]=3.72

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