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Art [367]
3 years ago
5

Consider the following reaction

Chemistry
1 answer:
andreyandreev [35.5K]3 years ago
8 0

Answer:

H2

Explanation:

CO2 + H2 → CO + H2O

↓ (-2). 0. (+2 )(-2). (+1)(-2)

↓ ·2 (+2)

+4 (-4)

Write down the oxidation number under each element, each molecule should equal 0 unless there is a charge shown.

Oxygen, always has an oxidation number of -2 unless in a peroxide.

Hydrogen, is -1 with metals,+1 with non-metals. Hydrogen loves non-metals!

H2 is zero because any standalone element has an oxidation number of zero

What is being oxidized? Whatever is being oxidized, loses electrons and becomes more positive, it will be a whole molecule, not just an element. In this case, the H in H2 goes from 0 to (+1) so it is the oxidized molecule.

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Element X is in group 2, and element Y is in group 7, of the periodic table. which ions will be present in the compound formed w
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2 years ago
Consider the reaction of NO and CO to form N2 and CO2, according to the balanced equation: 2 NO (g) + 2 CO (g) → N2 (g) + 2 CO2
Gekata [30.6K]

The image is not given in the question, it is attached below:

<u>Answer:</u> The excess reactant is NO, the limiting reactant is CO and the products are shown in the image attached below.

<u>Explanation:</u>

In the given image:

Red spheres represent oxygen atoms, blue spheres represent nitrogen atoms and black spheres represent carbon atoms

The combination of 1 black and 2 red spheres will represent carbon dioxide (CO_2) compound

The combination of 2 blue spheres will represent nitrogen molecule (N_2)

The combination of 1 blue and 1 red sphere will represent nitrogen monoxide (NO) compound

The combination of 1 black and 1 red sphere will represent nitrogen monoxide (NO) compound

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

We are given:

Given moles of NO = 6 moles

Given moles of CO = 4 moles

For the given chemical equation:

2NO(g)+2CO(g)\rightarrow N_2(g)+2CO_2(g)

By stoichiometry of the reaction:

If 2 moles of CO reacts with 2 moles of NO

So, 4 moles of CO will react with = \frac{2}{2}\times 4=4mol of NO

As the given amount of NO is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.

Thus, CO is considered a limiting reagent because it limits the formation of the product.

Hence, the excess reactant is NO, the limiting reactant is CO and the products are shown in the image attached below.

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3 years ago
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a.  mixtures are created through physical changes and compounds are created through chemical reactions

Explanation:

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