How do you see the use of nuclear energy? formulate a concise and clear opinion.

Chemistry

1 answer:

solong [7]3 years ago

5 0

Explanation:

Nuclear energy and technology are used within food and agriculture to make processes safer and more effective. For example, nuclear-related technologies are used in sterilizing agricultural pests to reduce the use of pesticides. This makes it impossible for the bugs to reproduce, gradually eliminating them.

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How much of Earth's atmosphere is made up of nitrogen and oxygen?

Archy [21]

<span>The right answer is the option B. Close to 99 percent. The atmosphere is a mixture of gases: nitrogen, oxygen, CO2, H2O, argon, among others. Nitrogen is about 78% and oxygen is about 21%, so they two together constitute about 99 percent of the Earth's atmosphere.</span>

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3 years ago

Read 2 more answers

Given the balanced equation 2C4H10 + 13O2 → 8CO2 + 10H2O, how many moles of CO2 are produced when 14.9g of O2 are used?

Anna [14]

Answer: The number of moles of $CO_2$ produced are, 0.287 moles.

Explanation : Given,

Mass of $O_2$ = 14.9 g

Molar mass of $O_2$ = 32 g/mol

First we have to calculate the moles of $O_2$

$\text{Moles of }O_2=\frac{\text{Given mass }O_2}{\text{Molar mass }O_2}$

$\text{Moles of }O_2=\frac{14.9g}{32g/mol}=0.466mol$

Now we have to calculate the moles of $CO_2$

The balanced chemical equation is:

$2C_4H_{10}+13O_2\rightarrow 10H_2O+8CO_2$

From the reaction, we conclude that

As, 13 mole of $O_2$ react to give 8 moles of $CO_2$

So, 0.466 mole of $O_2$ react to give $\frac{8}{13}\times 0.466=0.287$ mole of $CO_2$

Therefore, the number of moles of $CO_2$ produced are, 0.287 moles.

3 0

3 years ago

Find and fix each mistake in the following equilibrium constant expressions.

IRINA_888 [86]

Answer:

A. c. Keq=[H2]^2[S2]/[H2S]^2

B. b. Keq=[COCl2]/[CO][Cl2]

Explanation:

Hello,

In this case, considering the law of mass action which states that the equilibrium expression is written in terms of the concentration of products divided by the concentration of reactants considering the stoichiometric coefficients as powers we obtain:

A. For the reaction:

$2H_2S(g)\rightleftharpoons 2H_2(g)+S_2(g)$