00:01
Our chemical reaction is potassium hydroxide, koh, with nitric acid, hno3, producing kno3 and h2o.
00:17
So, because the stoichiometry is 1 to 1, and we have equal amounts, 100 milliliters at 0 .050 molar of both koh and hno3, then both reactants are consumed completely.
00:40
Both are, if you will, limiting reactants.
00:43
To determine the molar enthalpy of neutralization, delta h is equal to q for the reaction divided by the moles of either koh or hno3 because they're both the same.
01:02
Q of the reaction is equal to negative q of the solution.
01:10
Why negative? because when the reaction releases heat, the solution absorbs heat so their signs need to be different.
01:19
Q of the solution will be the specific heat of the solution.
01:23
We'll assume it's the same as water, 4 .184 joules per gram degrees celsius, multiplied by the mass of the solution.
01:34
If we mix 100 milliliters with 100 milliliters, and they're both mostly water, we can assume a density of 1 gram per milliliter.
01:43
So at two total, 200 total milliliters, we would have 200 total grams, which we then multiply by the change in temperature.
01:53
The final temperature, 21 .34 minus the initial temperature, 21 .01, and we get a release because it's negative of 276 joules or negative 0 .276 kilojoules...