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Wewaii [24]
3 years ago
5

Use the problem below to answer the question: How many grams of H2 would be formed if 34 grams of carbon reacted with an unlimit

ed amount of H2O? The reaction is: C + H2O → CO + H2 The equation is balanced. The starting substance is carbon, C. The ending substance is hydrogen, H2. Using the periodic table, find the molecular mass of H2. H2 = g/mole
Chemistry
2 answers:
Pavlova-9 [17]3 years ago
6 0
34g C * ( 1 mol / 12.0107 ) * ( 1 mol H2 / 1 mol C ) * ( <span>2.01588 g / 1 mol H2 ) = 5.70657164028741 g H2 = 5.7 g H2

Convert grams of C to moles of C using the given amount of grams and the molar mass ( 12.0107 g/mol ).

Gather the mole ratio from the coefficients in the balanced equation and multiply by the ratio.

Convert moles of H2 to grams of H2 </span> using the given amount of grams and the molar mass ( 2.01588 g/mol )<span>.

Revise your answer to have the correct number of significant figures. </span>
Aleksandr [31]3 years ago
5 0

<u>Answer:</u> The mass of hydrogen gas formed will be 5.66 g

<u>Explanation:</u>

To calculate the number of moles, we use the formula:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}    .....(1)

<u>For Carbon:</u>

Given mass = 34 g

Molar mass = 12 g/mol

Putting values in above equation, we get:

\text{Moles of carbon}=\frac{34g}{12g/mol}=2.83mol

For the given chemical equation:

C+H_2O\rightarrow CO+H_2

By Stoichiometry of the reaction:

1 mole of carbon produces 1 mole of hydrogen gas.

So, 2.83 moles of carbon atom will produce = \frac{1}{1}\times 2.83=2.83mol of hydrogen gas.

Now, to calculate the mass of hydrogen gas, we use equation 1.

Moles of Hydrogen gas = 2.83 mol

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

2.83mol=\frac{\text{Mass of Hydrogen gas}}{2g/mol}\\\\\text{Mass of Hydrogen gas}=5.66g

Hence, the mass of hydrogen gas formed will be 5.66 g

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tresset_1 [31]

Answer:

Mg ²⁺

Explanation:

Τhe metal loses electrons and in forming Mg²⁺ ,it loses 2 electrons and hence oxidized.

Mg(s) ⇒ Mg²⁺ + 2e⁻

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3 years ago
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Answer:

2.14 moles of H₂O₂ are required

Explanation:

Given data:

Number of moles of H₂O₂ required = ?

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Solution:

Chemical equation:

N₂H₄  +   2H₂O₂       →   N₂ +  4H₂O

now we will compare the moles of H₂O₂ and N₂H₄

                          N₂H₄     :      H₂O₂  

                            1           :        2

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3 years ago
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oxidation-reduction reactions are -

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For reaction,

  1. 2C3H6(g) + 9O2(g) → 6CO2(g) + 6H2O(g)

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<u>On product side:</u>

Oxidation state of Carbon = +4

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Here, carbon's oxidation state is rising from +2 to +4. As a result, it is oxidizing and the oxygen's oxidation state is decreasing from 0 to -2. As a result, it is decreasing.

For reaction,

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<u>When reacting:</u>

Iron's oxidation state is +3.

Carbon's oxidation state is +2.

<u>On product side:</u>

Iron's oxidation state is zero.

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Here, carbon's oxidation state is rising from +2 to +4. As a result, it is being oxidized and the iron's oxidation state is changing from +3 to 0. As a result, it is decreasing.

To learn more about oxidation-reduction from given link

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