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Ilia_Sergeevich [38]
3 years ago
11

Assume 3 molecules of Fe react according to the following equation. 3Fe + 4H2O Fe3O4 + 4H2 How many molecules of H2 are produced

? How many water molecules are required? What is the mole ratio of Fe to H2O? How many hydrogen molecules (H2) are involved in this reaction?
Chemistry
2 answers:
user100 [1]3 years ago
6 0

How many molecules of H2 are produced?: 4 molecules

How many water molecules are required?: 4 molecules

What is the mole ratio of Fe to H2O?: 3/4

How many hydrogen molecules (H2) are involved in this reaction?: 4 molecules

Wewaii [24]3 years ago
5 0
Chemical reaction:  3Fe + 4H₂O → Fe₃O₄ + 4H₂<span>.
From chemical reaction:
1) n(Fe) : n(H</span>₂) = 3 : 4.
Four molecules of hydrogen are produced.
2) n(Fe) : n(H₂O) = 3 : 4.
Four molecules of water are required, because the mole ratio of Fe to H₂O is 3:4.
3) Hydrogen molecules are not<span> involved in this reaction, but produced (4 molecules).</span>
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What mass of butane in grams is necessary to produce 1.5×103 kj of heat what mass of co2 is produced?
kari74 [83]
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C_{4} H_{10} + \frac{13}{2} O_{2} ---> 4 CO_{2}  + 5 H_{2}O

The mass of butane required in the reaction is based on the heat produced by the reaction, which is given to be -1,500 kJ. The minus sign is added because the reaction releases heat (exothermic), which means that the products are in a "lower energy state" than the reactants. 

Dividing this with the heat of reaction per mole of butane reacted would give the number of moles butane required. Then, multiplying the answer with the molar mass of butane which is 58 grams/mole, will give the mass of butane required. 

Moles of butane = [(-1,500 kJ)/(-2658 kJ/mol butane)]
Moles of butane = 0.5643 moles butane

Mass of butane  = 0.5643 moles butane * 58 grams/mol butane
Mass of butane  = 32.73 grams butane

The mass of carbon dioxide (CO_{2}) can be determined by multiplying the moles of butane (C_{4} H_{10}) with the mole ratio of (CO_{2}) produced to the (C_{4} H_{10}) reacted, and then with the molar mass of (CO_{2}), which is 44 grams/mole. 

Mass of carbon dioxide produced 
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Mass of carbon dioxide produced  
    = 99.32 grams CO_{2}

Thus, the mass of butane required is 32.73 grams, and the mass of carbon dioxide produced from the reaction of this amount of butane is 99.32 grams. 
                
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lakkis [162]
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2FeBr3(aq) + 3Na2S(Aq) --> Fe2S3(s) + 6NaBr(aq)   [original eqation]

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3 years ago
Balance the following
olga55 [171]

Answer:

Your coefficients (the numbers in front of the molecule) will be the following from left to right.

1. <u>1 - 2 - 1 - 2</u>

2. <u>2 - 1 - 2 - 2 - 1</u>

3. <u>2 - 4 - 1</u>

4. <u>2 - 4 - 3</u>

5. <u>2 - 2 - 2 - 1</u>

6. <u>1 - 1 - 1</u>

7. <u>2 - 1 - 2</u>

8. <u>3 - 1 - 2 - 3</u>

9. <u>3 - 1 - 2 - 3</u>

10. <u>2 - 1 - 1 - 1</u>

Explanation:

To balance this equations first count how many times an element is on each side and then see what needs to be changed in order to balance them.

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