2H2+O2 -> 2H20 changeHrxn=-484 KJ
Which answer best describes the transfer heat that occurs when 1.30 mol of H2 reacts?
629 KJ released
315 KJ absorbed
315 KJ released
484 KJ absorbed
484 KJ released
629 KJ absorbed
315 released
The sign is negative which means the heat is released. That makes three answers (absorbed) go away.
(484/2 mol) x 1.3 mol = ?
Well, well, well, let's see what we have here. According to the chemical equation provided, the reaction releases 484 KJ of heat when 2 moles of H2 react. So, let's do some math magic!
If 2 moles of H2 release 484 KJ, how much do you think 1 mole of H2 will release? It's like a good old-fashioned proportion problem!
If we divide 484 KJ by 2, we get 242 KJ. But hold your horses, we're not done yet! We need to find out how much heat is released by 1.30 moles of H2.
So, if 1 mole of H2 releases 242 KJ, and we have 1.30 moles of H2, how much heat will be released?
Drumroll, please! Multiply 242 KJ by 1.30, and you get... 314.6 KJ.
But remember, I don't do decimals, so let's round that up to the nearest whole number.
So, my comedic friend, the correct answer is 315 KJ released! Ta-da!
To determine the transfer of heat that occurs when 1.30 mol of H2 reacts, we need to use the given equation and its change in enthalpy (∆Hrxn = -484 KJ).
Given that the stoichiometric coefficient of H2 is 2 in the balanced equation, we can calculate the moles of H2 involved in the reaction as follows:
1.30 mol H2 × (1 mol H2 / 2 mol H2) = 0.65 mol H2
Now, we can use the stoichiometry of the reaction to find the transfer of heat. Since the stoichiometric coefficient of H2 is 2 in the balanced equation, we need to multiply the change in enthalpy by the moles of H2:
0.65 mol H2 × (-484 KJ / 2 mol H2) = -315.8 KJ
The negative sign indicates that heat is being released or given off by the reaction. Therefore, the correct answer is:
315 KJ released.