An unknown compound is processed using elemental analysis and found to contain 117.4 g of platinum, 28.91 g of carbon, and 33.71
1 answer:
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Answer : The enthalpy of reaction is, 67.716 KJ/mole
Explanation :
First we have to calculate the moles of and
.
Now we have to calculate the moles of AgCl formed.
The balanced chemical reaction will be,
As, 1 mole of react with 1 mole of
to give 1 mole of
So, 0.005 mole of react with 0.005 mole of
to give 1 mole of
The moles of AgCl formed = 0.005 mole
Total volume of the solution = 50.0 ml + 50.0 ml = 100.0 ml
Now we have to calculate the mass of solution.
Mass of the solution = Density of the solution × Volume of the solution
Mass of the solution = 1.00 g/ml × 100.0 ml = 100 g
Now we have to calculate the heat.
where,
q = heat
C = specific heat capacity =
m = mass = 100 g
= final temperature =
= initial temperature =
Now put all the given values in the above expression, we get:
Now we have to calculate the enthalpy of the reaction.
where,
= enthalpy of reaction = ?
q = heat of reaction = 338.58 J
n = moles of reaction = 0.005 mole
Now put all the given values in above expression, we get:
Conversion used : (1 KJ = 1000 J)
Therefore, the enthalpy of reaction is, 67.716 KJ/mole