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1 year ago

calculate the mass of HNO3 obtained when 20.0g of KNO3 reacts completely with excess concentrated H2SO4

Chemistry

1 answer:

iragen [17]1 year ago

8 0

The mass of HNO3 obtained is 12.46 g from the given reaction.

The chemical reaction is :

Potassium Nitrate + Sulphuric acid ------> Potassium Bisulphate + Nitric acid.

The above reaction is basically used for the making of nitric acid.

Less than 200 degree celcius the Nitric acid if more than 200 degree celcius then it will form Potassium Sulphate.

Now,

1 mol of KNO3 reacts with1 mol of concentrated H2SO4 to give 1 mol HNO3

Molar Mass of KNO3 = 101.1 g

Molar mass of H2SO4 = 98.07 g

Mass of H2SO4 that can react with 20 g of KNO3 = (20 g* 98.07 g )/ 101.1 g

= 19.4 g

Molar mass of nitric acid= 63.01 g

Hence mass of nitric acid produced by 20 g of KNO3 = (20 g * 63.01 g ) / 101.1 g = 12.46 g

To know more about Nitric acid here :

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Consider the combustion of octane (C8H18)

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The balanced equation for the above reaction is as follows;
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when 2 mol of octane reacts it forms 16 mol of CO₂
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3 years ago

Which of the following is a chemical change? Explain your reasoning: (a) boiling canned soup; (b) toasting a slice of bread; (c)

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Answer:

(d) burning a log.

(b) toasting a slice of bread;

Explanation:

Chemical change -

A chemical change refers to , the change in which a new compound is formed .

From the question ,

boiling canned soup ,

Its is not a chemical process , since no new compound is formed , these is only change in state as the liquid is turning to gaseous sate .

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It is not a chemical process , as no new substance is formed .

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Nitrogen forms a surprising number of compounds with oxygen. A number of these, often given the collective symbol NOx (for "nitr

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Answer:

9.2

Explanation:

Let's do an equilibrium chart of this reaction:

2NO(g) + O₂(g) ⇄ 2NO₂(g)

4.9 atm 5.1 atm 0 Initial

-2x -x +2x Reacts (stoichiometry is 2:1:2)

4.9-2x 5.1-x 2x Equilibrium

The mole fraction of NO₂ (y) can be calculated by the Raoult's law, that states that the mole fraction is the partial pressure divided by the total pressure:

y = 2x/(4.9 - 2x + 5.1 -x + 2x)

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2.52x = 5.2

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Thus, the pressure equilibrium constant Kp is:

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