In an experiment a 03792 g sample of azulene c10h8 is burned...

In an experiment, a 0.3792 g sample of azulene (C10H8) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.280×103 g of water. During the combustion, the temperature increases from 22.45 to 25.09 °C. The heat capacity of water is 4.184 J/g°C. The heat capacity of the calorimeter was determined in a previous experiment to be 775.6 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of azulene based on these data. C10H8(s) + 12O2(g) → 4H2O(l) + 10CO2(g) + Energy Molar Heat of Combustion = kJ/mol

Transcript

00:01 Hi, in this question we have to calculate the heat of combustion of the reaction.

00:05 Now firstly, the energy lost by this during this reaction is absorbed by water and calorimiter.

00:13 So let it be q, that is, heat absorbed.

00:19 So now this heat absorbed will be equal to heat absorbed by water plus heat absorbed by the calorimeter.

00:27 So now it can be written as, now heat absorbed by water is mass multiply by, specific heat of water multiply by change in temperature plus heat absorbed by calorimeter will be equal to calorie meter constant multiply by temperature change so now mass of water is equal to 1 .280 into 10 raised to power 3 gram given and now delta t is equal to t final that is final temperature minus initial temperature which is equal to 25 .09 degrees celsius minus 22 .45 degrees celsius.

01:08 So it is equal to 2 .64 degrees celsius.

01:13 And cw value is given to us and calorimeter constant is also.

01:18 So from here q is equal to now mass is 1 .280 into 10 raised to power 3 gram multiplied by 4 .184 jowl per gram per degree celsius, multiplied by 2 .64 degrees celsius, plus 775 .6 jowl per degree celsius, multiply by 2 .64 degrees celsius.

01:43 So on calculating this, we get the heat absorbed as equal to 141 .38 .57 jowl.

01:53 Now, 1 jowl is equal to 10 raise to power minus 3 kilojoules.

02:01 So from here, heat absorbed is equal to 14138 .57 multiply by 10 raised to power minus 3 kilojoules.

02:10 So it is equal to 14 .14 kilojoules.

02:15 Now, according to calorimetry principle, heat lost is equal to minus heat absorbed.

02:25 So, that is, heat lost is the heat loss during the reaction...