Question

I know this isn't chemistry but no one is ever there to help so can someone help me with this problem...

The energy diagram shown represents the chemical reaction between solid ammonium chloride and solid barium hydroxide octahydrate:

2NH4Cl(s) + Ba(OH)2 x 8H2O(s)---->2NH3(aq)+BaCl2(aq)+10H2O(1)

The (triangle then an H) for this reaction is 54.8 kJ. How much energy would be absorbed if 23.7 g of NH4Cl reacts?

Answer 1

i tried one way it didnt work give me 5 minutes ill try to solve it

Answer 2

okay so first convert 23.7 g into moles
23.7g-x moles of NC4Cl
157g- 1 mole NC4Cl
solve for x (23.7x1)/157
23.7g=0.15 moles

now for 2 moles- 54.8 kj
for 0.15-x kj
solve for x (54.8x0.15)/2
so 4.11 kj for 23.7g.

I'm not sure if this is right, I took chem 2 years ago, but hopefuly it helps

Answer 3

Moles of NH4Cl: 23.7 / 53.5 = .443 mol
Energy absorbed: .443 * 54.8 Kj/ 2 = 12.1 Kj

Answer 4

oh, okay yeah that looks more correct

Answer 5

you should know that just multiply by mole!

Answer 6

The energy diagram shown represents the chemical reaction between solid ammonium chloride and solid barium hydroxide octahydrate:
2NH 4 Cl(s)+Ba(OH) 2 ⋅8H 2 O(s)→2NH 3 (aq)+BaCl 2 (aq)+10H 2 O(l) \rm 2NH_4Cl(s) + Ba(OH)_2\cdot8H_2O(s) \rightarrow 2NH_3(aq) + BaCl_2 (aq) + 10H_2O(l)
The ΔH Delta H for this reaction is 54.8kJ kJ . How much energy would be absorbed if 25.3g g of NH 4 Cl \rm NH_4Cl reacts