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Calcium carbide is used for the artificial ripening of fruits. Actually, the fruit ripens because of the heat evolved while calcium carbide reacts with moisture. During the reaction, calcium hydroxide and acetylene gas is formed.

If 200 cm3 of acetylene is formed from a certain mass of calcium carbide. Find the volume of oxygen required and carbon dioxide formed during the complete combustion. The combustion reaction can be represented as below:

2C2H2(g)+5O2(g)4CO2(g)+2H2O(g)


A

500 cm3 of oxygen is required and 350 cm3 of CO­2 is formed.

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B

500 cm3 of oxygen is required and 400 cm3 of CO­2 is formed.

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C

450 cm3 of oxygen is required and 350 cm3 of CO­2 is formed.

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D

450 cm3 of oxygen is required and 400 cm3 of CO­2 is formed.

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Solution

The correct option is B

500 cm3 of oxygen is required and 400 cm3 of CO­2 is formed.


2C2H2(g)2 vol.+5O2(g)5 vol4CO2(g)4 vol.+2H2O(g)

From the equation, we have 2 vol. of acetylene requires 5 vol. of oxygen.

1 vol. of acetylene will require 52 vol. of oxygen.

200 cm3 of acetylene will require 52×200=500 cm3 of oxygen.

Again, 2 vol. of acetylene is required to form 4 vol. of CO2

1 vol. of acetylene will be required to form 4/2 vol. of CO2

200 cm3​ of acetylene will be required to form 42×200=400 cm3 of CO2​.

Hence, 500 cm3​ of oxygen is required and 400 cm3​ of CO2​ is formed.


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(a) A gas cylinder of capacity of 20dm3 is filled with gas X the mass of which is 10 g. When the same cylinder is filled with hydrogen gas at the same temperature and pressure the mass fo the hydrogen is 2 g, hence the relative molecular mass of the gas is :
(i) 5 (ii) 10 (iii) 15 (iv) 20
(b) (i) Calcium carbide is used for the artificial ripening of fruits. Actually the fruit ripens beause fo the heat evolved while calcium carbide reacts with and acetylene gas is formed. If 200cm3 of acetylene is formed from a certain mass of calcium carbidem, find the volume of oxygen required and carbon dioxide formed during the complete combustion. The combustion reaction can be represented as below.
2C2H2(g)+5O2(g)4CO2(g)+2H2O(g)
(ii) A gaseous compound of nitrogen and hydrogen contains 12.5% hydrogenj by mass. Find the molecular formula of the ocmpound if its relative molecular mass is 37.[N=14,H=1].
(c) (i) A gas cylinder contains 24×1024 moleules of nitrogen gas. If avogadro's number is 6×1023 and the relative atomic mass of nitrogen is 14, calculate:
(1) Mass of nitrogen gas in th ecylinder
(2) Volume of nitrogen at STP in dm3
(ii) Commercial sodium hydroxide wieghing 30 g has some sodium chloride in it. The mixture on dissolving in water and subsequent treatment with excesss silver nitrate solution formed a precipitate weighing 14.3 g. What is the percentage fo sodium chloride in the commercial sample of sodium hydroxide? The equation for the reaction is
NaCl+AgNO3AgCl+NaNO3
[Relative molecular mass of NaCl=58;AgCl=143]
(iii) A certain Gas 'X' occupies a volume of 100cm3
at S.T.P. and weighs 0.5 g. Find its relative moleular mass.

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