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:

link

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,

for step 7 table c on the lab "newtons law of action"   the average time it took the car to travel .25 meters   was 1.92 seconds.

the average time it took the car to travel 0.50 meters was 2.61 seconds

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