Question
Look at the reaction used to produce ammonia below. Calculate the energy released by forming bonds in this reaction. Use the table to help you. Enter your answer as a number mathrm(kJ) / mathrm(mol) [ mathrm(N)_(2)+3 mathrm(H)_(2) arrow 2 mathrm(NH)_(3) ] Bond & Bond energy mathrm(kJ) / mathrm(mol) mathrm(H)-mathrm(H) & 436 mathrm(O)-mathrm(O) & 498 mathrm(H)-mathrm(O) & 454 mathrm(C)-mathrm(H) & 413 mathrm(C)=mathrm(O) & 803 mathrm(N) mathrm(NH) & 945 mathrm(N)-mathrm(H) & 391 mathrm(O)-mathrm(O) & 243 mathrm(H)-mathrm(Cl) & 432
Answer
4.3
(197 Votes)
Greta
Master · Tutor for 5 years
Answer
The energy released is \( (2 \times 391 \times 3) \) kj/mol =
kj/mol. Formula used:###
.### Completing this calculation, ###
.
Explanation
## Step1:The energy released from forming a bond refers to the quantity of energy that is released (this is exothermic energy) when new chemical bonds form in the product molecules. For this reaction, the chemical product is ammonia (NH3). ## Step2:From the table, the bond energy of a single
bond is 391 kJ/mole.## Step3: However, we notice that there are three nitrogen-hydrogen (N-H) bonds within one molecule of NH3. Thus, the total chemical amount is multiplied by three. Therefore, the energy released will be
.## Step4:According to the balanced chemical equation, two molecules of NH3 are formed for every one molecule of N2 and three molecules of H2. Thus, the total amount of energy released when two moles of ammonia react is \( (2 \times \mathrm{NH} \times 3) \). Calculate this total energy.