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3 years ago

How does energy from the sun affect the motion of molecules in a gas compared to molecules in a liquid?

Biology

1 answer:

suter [353]3 years ago

6 0

Answer:

Molecules of gas starts movement when they get energy from the sun in the form of heat.

Explanation:

Molecules of gas absorbed heat energy coming from sun. This heat energy is converted into kinetic energy due to which gas molecule moves faster. Volume of gas molecules also increases due to expansion of molecules by the absorption of heat energy. So more space is occupied by gas molecule as compared to liquid molecules.

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3 years ago

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7) Calculate ∆G^0' for the following reaction: glucose + 6O2 → 6 CO2 + 6 H2O. Is this reaction exergonic or endergonic?

san4es73 [151]

The reaction is endergonic.

<h2>Procedure - Determination of the Gibbs reaction type</h2>

<h3>Thermochemical model</h3>

First, we need to determine the Gibbs free energy function ( $\Delta G_{o}$ ), in kilojoules, of the entire reaction by this formula:

$\Delta G_{o} = \Sigma\limits_{j=1}^{m} n_{j}\cdot g_{o, j} - \Sigma\limits_{i=1}^{p}n_{i}\cdot g_{o,i}$ (1)

Where:

$n_{i}$ - Number of kilomoles of the i-th reactive, in kilomoles.
$n_{j}$ - Number of kilomoles of the j-th product, in kilomoles.
$g_{o,i}$ - Specific Gibbs free energy function of the i-th reactive, in kilojoules per kilomole.
$g_{o,j}$ - Specific Gibbs free energy function of the j-th reactive, in kilojoules per kilomole.

<h3>Data from thermochemical tables</h3>

From thermochemical tables we have the following information:

Reactives

$g_{glu} = -2871596\,\frac{kJ}{kmol}$ , $g_{O_{2}} = 0\,\frac{kJ}{kmol}$

$n_{glu} = 1\,kmol$ , $n_{O_{2}} = 6\,kmol$

Products

$g_{CO_{2}} = -137150\,\frac{kJ}{kmol}$ , $g_{H_{2}O} = -237180\,\frac{kJ}{kmol}$

$n_{CO_{2}} = 6\,kmol$ , $n_{H_{2}O} = 6\,kmol$

<h3>Determination of the Gibbs free energy function</h3>

Now we proceed to determine the Gibbs free energy function and later determine the nature of the <em>thermochemical</em> reaction:

$\Delta G_{o} = (6\,kmol)\cdot \left(-137150\,\frac{kJ}{kmol} \right) + (6\,kmol)\cdot \left(-237180\,\frac{kJ}{kmol} \right)-(1\,kmol)\cdot \left(-2871596\,\frac{kJ}{kmol} \right) - (6\,kmol)\cdot \left(0\,\frac{kJ}{kmol} \right)$

$\Delta G_{o} = 625616\,kJ$

The Gibbs free energy function of the <em>entire</em> reaction is 625616 kilojoules.

<h3>Analysis of the result</h3>

The Gibbs free energy function has a <em>positive</em> sign, which means that this reaction is endergonic.

To learn more on Gibbs free energy, we kindly invite to check this verified question: brainly.com/question/9552459

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2 years ago