An empty water bottle is full of air at 15°C and standard pressure. The volume of the bottle is 0.500 liter. How many moles of a
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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 :
<u>Part 1 :</u>
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 =
<u>Part 2 :</u>
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,
<u>Part 3 :</u>
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:
<u>Part 4 :</u>
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