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gogolik [260]
3 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]3 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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Consider this reaction: NH4 HPO42− → NH3 H2PO4− Which is the Bronsted-Lowry acid ? NH4 HPO42- HPO42– H2PO4–.
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Bronsted - Lowry acid in the given reaction is NH₄, as it gives H⁺ ion.

<h3>What is Bronsted - Lowry acid?</h3>

According to the theory of Bronsted - Lowry, acids are those substances which gives H⁺ ion or proton in the aqueous medium.

Given chemical reaction is :

NH₄ + HPO₄²⁻ → NH₃ + H₂PO₄⁻

In the above reaction NH₄ is the Bronsted - Lowry acid as it gives H⁺ ion in the reaction and changes to NH₃ which is the conjugate base of NH₄. Whereas HPO₄²⁻ is the  Bronsted - Lowry base as it accepts the H⁺ ion to form H₂PO₄⁻ which is the conjugate acid of it.

Hence, option (1) is correct, i.e. NH₄ is the Bronsted - Lowry acid.

To know more about Bronsted - Lowry acid, visit the below link:

brainly.com/question/1435076

8 0
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What periodic pattern are noticed for the charges on the ions
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How many moles of oxygen molecules are present in 112ml of co2 at NTP?​
dexar [7]

In each mole of carbon dioxide there will be one mole of O₂.

Let us calculate the moles of carbon dioxide gas present first

The conditions are NTP it means , Temperature = 293 K and P = 1 atm

We will use ideal gas equation

PV= nRT

Where

P = Pressure of gas = 1 atm

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Putting values

moles=\frac{PV}{RT}=\frac{1X0.112}{0.0821X293}

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Thus moles of carbon dioxide will be 0.00466

The moles of O₂ = 0.00466

7 0
3 years ago
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