Answer:
The enthalpy change per mole of Mg is (ΔH) = 460 kj mol⁻¹
Explanation:
the total volume of the solution is
100 ml, its mass is (100 ml)(1.0 g ml⁻¹) = 100 g (Density of water 1 g ml⁻¹)
The temperature change is ΔT = 11.1 ∘C
Heat of reaction = Cs × m × ∆T
= (4.18 Jg⁻¹ ∘C⁻¹)(100 g)(11.1 ∘C)
= 4639.8 j = 4.6 kJ
Because the process occurs at constant pressure, ΔH = qP = 4.6 kJ
To express the enthalpy change on a molar basis
Mole of Mg = = 0.01 mol
Thus, the enthalpy change per mole of Mg is ΔH = = 460 kj mol⁻¹
Answer:
I think it should be Carbon.
Answer:
The solution is given below
Explanation:
Heat, q= mc∆T
q= 125g x 4.18 J/g∙°C x (21.18x- 24.28) °C
q= -1619.75J
NEGATIVE SIGN INDICATES THAT HEAT IS ABSORBED.
Enthalpy Change, ∆H = 1619.75 7/ 10.5 g
= 154.26 J/g
No. of moles of KBr = Mass of KBr/ Molecular Weight of KBr
=10.5g/119gmol-1
=0.088 mol
∆H= 1619.75 J/ 0.088 mol
= 18.41 kJ/mol
You might want to elaborate on this