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gogolik [260]
2 years ago
5

a sample of an oxide of iron was reduced to iron by heating with hydrogen. the mass of iron obtained was 4.35g and mass of water

is 1.86g. deduce the equation for the reaction occurred.​
Chemistry
1 answer:
Hitman42 [59]2 years ago
5 0

Answer:

FeO(s) + H2(g)→ Fe(s) + H2O(g)

Explanation:

Moles of Iron will be = 4.35 g/55.845 g/mol

                                  = 0.0786 moles

Moles of water = 1.86 g/18 g/mol

                         = 0.103 moles

The mole ratio of Iron to water

= 0.0786 : 0.103

= 1   :  1.3

= 1 : 1

Therefore, the equation for the reaction is;

FeO(s) + H2(g)→ Fe(s) + H2O(g)

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6 0
1 year ago
In a synthesis reaction you start with 1.7L of Hydrogen how many liters of water will be produced?
jolli1 [7]

15.3 litres of water will be produced if we take 1.7 litres of Hydrogen

Explanation:

Let's take a look over synthesis reaction;

H_{2}+ O_{2}<u>                         </u>H_{2}O<u />

<u>Balancing the chemical reaction;</u>

2H_{2} +O_{2}<u>                        </u>2H_{2}O<u />

Thus, 2 moles of hydrogen molecules are required to form 2 moles of water molecules.

<u>Equating the molarity;</u>

<u />\frac{1.7*1}{2*2} = \frac{x*1}{2*18}

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x=\frac{1.7*2*18}{2*2}

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3 years ago
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7 0
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