If 2.50 grams of ethane is allowed to react with 5.00 grams of oxygen how many grams of water would be expected?

The mass of water produced is 4.29 g.

Explanation:

Given;

reacting mass of ethane, C₂H₆ = 2.5 g

reacting mass of oxygen, O₂ = 5.0 g

The balanced combustion reaction is given as follows;

2C₂H₆   +   7O₂ >  4CO₂    +   6H₂O

Based on the balanced equation above;

                                     requires

7.0 moles of oxygen >   2.0 moles of ethane

                                   requires

5.0 g of oxygen      >  x gram of ethane

x = (2 x 5) / 7

x = 1.43 g

Ethane is in excess of 1.07g (2.5 g - 1.43g)

Now, determine the mass of water produced by 1.43 g of ethane;

                                   requires

2.0 moles of ethane >   6.0 moles of water

                                   requires

1.43 g of ethane      >  y  gram of water

y = (6 x 1.43) / 2

y = 4.29 g

Therefore, the mass of water produced is 4.29 g.

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.

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