The heats of combustion of ethane (c2h6) and butane (c4h10) are 52 kj/g and 49 kj/g, respectively. we need to produce 1.000 x 103 kj heat by burning one of the fuels. which fuel will emit the least amount of co2? 1. calculate the number of grams needed of each fuel: 2. calculate the number of moles of each fuel: 3. write down the balanced chemical equation for the combustion of the fuels: 4. calculate the number of moles of co2 produced by burning each fuel to produce 1.000 x 103 kj. which fuel will emit the least amount of co2?

Answer :

(1) The number of grams needed of each fuel are 19.23 g and 20.41 g respectively.

(2) The number of moles of each fuel are 0.641 moles and 0.352 moles respectively.

(3) The balanced chemical equation for the combustion of the fuels.

(4) The number of moles of produced by burning each fuel is 1.28 mole and 1.41 mole respectively.

The fuel that emitting least amount of is

Explanation :

Part 1 :

First we have to calculate the number of grams needed of each fuel .

As, 52 kJ energy required amount of = 1 g

So, 1000 kJ energy required amount of =

and,

As, 49 kJ energy required amount of = 1 g

So, 1000 kJ energy required amount of =

Part 2 :

Now we have to calculate the number of moles of each fuel .

Molar mass of = 30 g/mole

Molar mass of = 58 g/mole

and,

Part 3 :

Now we have to write down the balanced chemical equation for the combustion of the fuels.

The balanced chemical reaction for combustion of is:

and,

The balanced chemical reaction for combustion of is:

Part 4 :

Now we have to calculate the number of moles of produced by burning each fuel to produce 1000 kJ.

From this we conclude that,

As, 1 mole of react to produce 2 moles of

As, 0.641 mole of react to produce moles of

and,

From this we conclude that,

As, 1 mole of react to produce 4 moles of

As, 0.352 mole of react to produce moles of

So, the fuel that emitting least amount of is

yes

explanation:

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