At 791 K and relatively low pressures, the gas-phase decompositio...

Question

At 791 K and relatively low pressures, the gas-phase decomposition 
of acetaldehyde 1CH3CHO2 is second order in 
acetaldehyde. 
CH3CHO1g2S CH41g2 + CO1g2 
The total pressure of a particular reaction mixture was 
found to vary as follows: 
<TABLE> 
(c) If the volume of the reaction mixture is 1.00 L, what 
is the total amount of heat liberated (in joules) after a 
reaction time of 605 s?

Accepted Answer

Hey everyone. Our question here is asking us to calculate the heat generated by the complete combustion of 6.32 kg of nitro Benzene for this question. We're going to go ahead and use our dimensional analysis and convert from kilograms of nitrobenzene into grams into moles of nitrobenzene and then finally into killing jewels of nitrobenzene. Starting off with 6.32 kg of Nitro Benzene, We can go ahead and convert this into Graham, since we know that one kg contains 10 to the 3rd g. And to convert from grams into moles, we can go ahead and use our molar mass of nitro Benzene, Which is 123.12 g per one mole and to convert from moles into killer jewels, we can go ahead and use our standard entropy of our reaction, which is 12352 kg jewels. And this is going to be perform away of Nitro Benzene. Since we have that coefficient of four prior to nitro Benzene in our balanced chemical reaction. And the reason why we got rid of our negative sign is because we're calculating the heat generated by our combustion. So when we calculate this out and cancel out our units, We're going to end up with a total of 1.5, 9 Times 10 to the 5th killer jewels. And this is going to be our final answer. So I hope this made sense. And let us know if you have any questions