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Given the reaction : 

C_{2}H_{5}OH\; +\; 3O_{2} \rightarrow\; 2CO_{2}\; +\; 3H_{2}O

How many grams of H2O is produced when 92g of C2H5OH is burnt?

  • Option 1)

    10.8

  • Option 2)

    108

  • Option 3)

    54

  • Option 4)

    72

 

Answers (1)

As we learnt.

Dalton's Atomic Theory -

Compounds are formed when atoms of different elements combine in a fixed ratio.

- wherein

N_{2} + 3H_{2} \rightleftharpoons 2NH_{3}

Nitrogen & Hydrogen combine in a fixed ratio to yeild ammonia (compound)

 

 

Molar mass of  C_{2}H_{5}OH = 2\times 12 +6\times 1 + 16 \times 1 = 46

Moles of C_{2}H_{5}OH = \frac{92}{46} = 2 moles

1 ml of C_{2}H_{5}OH gives 3 moles of H_{2}O

\therefore 2 ml of C_{2}H_{5}OH gives 6 moles of H_{2}O

\therefore H_{2}O produced = 6\times 18 = 108g

\therefore Solution is B


Option 1)

10.8

This is incorrect.

Option 2)

108

This is correct.

Option 3)

54

This is  incorrect.

Option 4)

72

This is  incorrect.

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subam

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