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USPshnik [31]
3 years ago
7

Oxyacetylene torches produce such high temperature that they are often used to weld and cut metal. When 1.53 g of acetylene (C2H

2) is burned in a bomb calorimeter with a heat capacity of 10.69 kJ/K, the temperature increases from 20.486°C to 44.688°C. What is ΔE (in kJ/mol) for this combustion reaction? Enter to 0 decimal places.
Chemistry
1 answer:
hodyreva [135]3 years ago
7 0

Answer: 4403kJ/mole

Explanation:

First we have to calculate the heat absorbed by bomb calorimeter  

Formula used :

q_b=c_b\times (T_{final}-T_{initial})

q_b = heat absorbed by calorimeter = ?

c_b = specific heat of = 10.69 kJ/K

T_{final} = final temperature = 44.688^oC=(273+44.688)K=317.688K

T_{initial} = initial temperature = 20.486^oC=(273+20.486)K=293.486K

q_b=10.69kJ/K\times (317.688-293.486)=258.7kJ

As heat absorbed by calorimeter is equal to the heat released by acetylene during combustion.

Thus 1.53 gram of acetylene releases heat of combustion = 258.7kJ

So, 26.04 g/mole of acetylene releases heat of combustion \frac{258.7}{1.53}\times 26.04=4403kJ/mole

Therefore, the heat of combustion of acetylene is, 4403kJ/mole

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Answer:

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