Oxyacetylene torches produce such high temperature that they are often used to weld and cut metal. when 1.53 g of acetylene (c2h2) 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.

The ΔE (in kJ/mol) for this combustion reaction is 4385 kJ/mol

We know that the number of moles = mass/molar mass

where;

From the given information, the number of moles of acetylene used:

= 1.53 g/26.04 g/mol

= 0.059 mol

When a given mass of fuel is burned in a bomb calorimeter with a known heat capacity, we can estimate the heat evolved during combustion by measuring the temperature change.

∴

Heat evolved = heat capacity × change in temperature

Heat evolved = 10.69 kJ/K × (44.688 - 20.486)K    

Heat evolved = 10.69 kJ/K ×  24.202K

Heat evolved = 258.719 kJ

We know that the heat of combustion ΔE is the amount of heat evolved by the complete combustion of 1 mole of a gas.

∴

Learn more about the heat of combustion here:

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Explanation:

First we have to calculate the heat absorbed by bomb calorimeter  

Formula used :

= heat absorbed by calorimeter = ?

= specific heat of = 10.69 kJ/K

= final temperature =

= initial temperature =

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

Therefore, the heat of combustion of acetylene is,

2b2t

explanation:

2b2t