What energy in kJ is required to break 4.24 mol of NH3 into atoms? As noted below, this information can be used to calculate ΔH for gas-phase reactions.
I got 1376.18, which is wrong.
All help is appreciated!
It would have helped if you had given the information "as noted below."
Look up the bond energy for N-H bond and times 3 will give you 1 mol NH3. Multiply that by 4.24.
True, sorry I forgot about that. I did what you said though and got it right, so thanks!
Well, breaking up relationships can be quite energy-consuming, even for molecules!
To calculate the energy required to break 4.24 mol of NH3 into atoms, you need to consider the bond energy of the N-H bond in ammonia (NH3). The bond energy is the energy required to break one mole of a particular bond in a compound.
In this case, the bond energy of the N-H bond in ammonia is around 392 kJ/mol. Since there are three N-H bonds in each ammonia molecule, you'll need to multiply the bond energy by three to calculate the energy required to break one ammonia molecule.
392 kJ/mol x 3 = 1176 kJ/mol
Now, multiply the energy required to break one ammonia molecule by the number of moles you have (4.24 mol) to get the total energy required:
1176 kJ/mol x 4.24 mol = 4982.24 kJ
So, the energy required to break 4.24 mol of NH3 into atoms is approximately 4982.24 kJ.
Hope this helps shed some light on the situation, though it's not the most funny. Chemistry can be a bit serious sometimes!
To calculate the energy required to break 4.24 mol of NH3 into atoms, we need to consider the bond energy of the NH3 molecule. The bond energy represents the energy required to break a specific bond.
The NH3 molecule consists of three N-H bonds. The average bond energy for the N-H bond is around 391 kJ/mol.
To break all the N-H bonds in one mole of NH3, you would need to supply 3 * 391 kJ = 1173 kJ of energy.
We know that we have 4.24 mol of NH3, so we will multiply the bond energy by this amount:
1173 kJ/mol * 4.24 mol = 4970.52 kJ
Therefore, the energy required to break 4.24 mol of NH3 into atoms is approximately 4970.52 kJ, not 1376.18 kJ.
To calculate the energy required to break a certain amount of NH3 molecules into atoms, we must consider the bond dissociation enthalpy (energy) for the N-H bond in NH3.
The balanced equation for the breaking of NH3 molecules into atoms is as follows:
4 NH3(g) → 4 N(g) + 12 H(g)
Given that 4.24 mol of NH3 is to be broken, we need to determine the number of N-H bonds present in 4.24 mol of NH3. Since each NH3 molecule has 3 N-H bonds, we can calculate the total number of N-H bonds as follows:
Number of N-H bonds = 4.24 mol × 3 N-H bonds/mol = 12.72 mol N-H bonds
Next, we need to find the bond dissociation enthalpy for the N-H bond. According to the data given, the bond dissociation enthalpy for the N-H bond in ammonia (NH3) is 391 kJ/mol.
To find the energy required to break all the N-H bonds, we multiply the number of N-H bonds by the bond dissociation enthalpy:
Energy required = 12.72 mol N-H bonds × 391 kJ/mol = 4970.32 kJ
Therefore, the correct answer is 4970.32 kJ, not 1376.18 kJ.