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3 years ago

Global bee populations have been declining over the past decade. What impact might this have on the world's human population?

Biology

1 answer:

aev [14]3 years ago

7 0

Answer:

Bees play a significant role in the field of agriculture. They can adapt to the process of pollination. Pollination is usually defined as the process of transportation of pollen grains from the male anther of a flower to the female stigma. The bees pollinate the crops and increases their productivity and yield capacity. About 35% of the food that we eat, are dependent on this pollination act that is carried out by the bees, involving either directly or indirectly.

Over the last few decades, the population of the bee has been decreasing, and it is directly affecting the global human population. It is because less amount of food is produced compared to the rate of demand, resulting in a shortage of food items.

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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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