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Ronch [10]
2 years ago
11

Using the equation 2H2+O2=2H2O, when 47g of water are produced, how many grams of hydrogen must react?

Chemistry
2 answers:
Fed [463]2 years ago
6 0

See , from the equation we can see that for forming two mole of H2O 2Mole of H2 has to react.

Mass of 2 Mole H2O is 18*2gm or 36gm.

So for forming 36 gm H2O 2×2 I.e. 4 gm H2 has to take part in reaction.

Therefore, to form 1 gm H2O 4÷36 gm of H2 has to take part.

So, for forming 47gm H2O (4÷36)×47 gm H2 has to take part

I.e. 5.22 gm of H2 has to take part

So, ans is 5.22 gm of hydrogen.

Hope it helps!!!

Katarina [22]2 years ago
5 0

<u>Answer:</u> Mass of hydrogen gas that must react will be 5.22 grams.

<u>Explanation:</u>

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

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

Given mass of water = 47 g

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

\text{Moles of }H_2O=\frac{47g}{18g/mol}=2.61mol

For the given balanced chemical equation:

2H_2+O_2\rightarrow 2H_2O

By Stoichiometry of the reaction:

2 moles of water are formed from 2 moles of hydrogen gas.

So, 2.61 moles of water will be formed from \frac{2}{2}\times 2.61=2.61mol of hydrogen gas.

Now, calculating the mass of hydrogen by using equation 1:

Moles of hydrogen gas = 2.61 moles

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

2.61mol=\frac{\text{Mass of hydrogen gas}}{2g/mol}\\\\\text{Mass of hydrogen gas}=5.22g

Hence, mass of hydrogen gas that must react will be 5.22 grams.

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Propane can be turned into hydrogen by the two-step reforming process. In the first step, propane and water react to form carbon
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Answer:

C₃H₈(g) + 6 H₂O(g) ⇒ + 10 H₂(g) + 3 CO₂(g)

Explanation:

Propane can be turned into hydrogen by the two-step reforming process.

In the first step, propane and water react to form carbon monoxide and hydrogen. The balanced chemical equation is:

C₃H₈(g) + 3 H₂O(g) ⇒ 3 CO(g) + 7 H₂(g)

In the second step, carbon monoxide and water react to form hydrogen and carbon dioxide. The balanced chemical equation is:

CO(g) + H₂O(g) ⇒ H₂(g) + CO₂(g)

In order to get the net chemical equation for the overall process, we have to multiply the second step by 3 and add it to the first step. Then, we cancel what is repeated.

C₃H₈(g) + 3 H₂O(g) + 3 CO(g) + 3 H₂O(g) ⇒ 3 CO(g) + 7 H₂(g) + 3 H₂(g) + 3 CO₂(g)

C₃H₈(g) + 6 H₂O(g) ⇒ + 10 H₂(g) + 3 CO₂(g)

4 0
3 years ago
The relative atomic mass of Chlorine is 35.45. Calculate the percentage abundance of the two isotopes of Chlorine, 35Cl and 37Cl
nata0808 [166]

Answer:

35Cl = 75.9 %

37Cl = 24.1 %

Explanation:

Step 1: Data given

The relative atomic mass of Chlorine = 35.45 amu

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37Cl = 36.96590258 amu

Step 2: Calculate percentage abundance

35.45 = x*34.96885269 + y*36.96590258

x+y = 1  x = 1-y

35.45 = (1-y)*34.96885269 + y*36.96590258

35.45 = 34.96885269 - 34.96885269y +36.96590258y

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y = 0.241 = 24.1 %

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Answer:

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Step 1:

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