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4 years ago

Solid carbon reacts with oxygen gas to form carbon dioxide gas . Write a balanced chemical equation for this reaction

Chemistry

2 answers:

alekssr [168]4 years ago

8 0

<u>Answer:</u> The chemical reaction is given below.

<u>Explanation:</u>

When solid carbon reacts with oxygen molecule, it leads to the production of carbon dioxide gas.

The chemical equation for the formation of carbon dioxide follows:

$C(s)+O_2(g)\rightarrow CO_2(g)$

By Stoichiometry of the reaction:

1 mole of solid carbon reacts with 1 mole of oxygen gas to produce 1 mole of carbon dioxide gas.

Nikitich [7]4 years ago

7 0

Solid carbon reacts with oxygen gas to form carbon dioxide gas.

The balanced chemical equation for this reaction:

$C (s) + O_{2}(g) ---> CO_{2}(g)$

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rewona [7]

Answer:

Tin(IV) Oxide + Carbon = Tin + Carbon Monoxide

Explanation:

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3 years ago

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Nuetrik [128]

Answer:

Dissociation of O-H bond is highly favorable in p-cyanobenzoic acid resulting to higher acidity as compared to m-cyanobenzoic acid.

Explanation:

In p-cyanobenzoic acid, adjacent carbon to carboxyl group (-COOH) gets a partial positive charge due to electron withdrawing resonating effect of carboxyl group as compared to m-cyanobenzoic acid.

Due to this partial positive charge on carbon atom in p-cyanobenzoic acid, O-H bond in -COOH group remains highly polarized towards oxygen atom. Hence, dissociation of O-H bond is highly favorable in p-cyanobenzoic acid resulting to higher acidity as compared to m-cyanobenzoic acid.

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3 years ago

CaCO3 → CaO + CO2 Calculate the theoretical yield of Calcium Oxide if 24.8 grams of Calcium Carbonate decomposes. Calculate the

RideAnS [48]

Answer:

Theoretical yield: 13.9 g

Percent yield: 94 %

Explanation:

The reaction is:

CaCO₃ → CaO + CO₂

We see that the reaction is correctly balanced.

1 mol of calcium carbonate can decompose to 1 mol of calcium oxide and 1 mol of carbon dioxide.

We convert the mass to moles: 24.8 g . 1mol / 100.08g = 0.248 moles

As ratio is 1:1, 0.248 moles of salt can decompose to 1 mol of oxide.

We convert the moles to mass: 0.248 mol . 56.08g /1mol = 13.9 g

That's the theoretical yield.

To determine the percent yield we think:

(Determined yield / Theoretical yield) . 100 → (13.1 / 13.9) . 100 = 94 %

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3 years ago

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You would have to use the ideal gas law for this:
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