Take a look at the thermochemical equation for the combustion of hexene gas shown below. If the reaction is conducted in a calorimeter containing 445 mL of water at 19 degrees celsius (initially) and a total of 7.4 grams of hexene (C6H12) is combusted, what will the final temperature of the water be? Assume the density of water is 1 g/mL and the specific heat capacity of water is 4.18 J/gC. Round your answer to 2 decimal places, if necessary. Do not include units in your final answer. C6H12(g) + 9O2(g) --> 6H2O(g) + 6CO2(g)
Hcombustion = -432.09kJ/mol

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

a is the correct answer