ΔHrxn = ΣδΗ(bond breaking) - ΣδΗ(bond making)
Bond enthalpies,
N ≡ N ⇒ 945 kJ mol⁻¹
N - Cl ⇒ 192 kJ mol⁻¹
Cl - Cl⇒ 242 kJ mol⁻¹
According to the balanced equation,
ΣδΗ(bond breaking) = N ≡ N x 1 + Cl - Cl x 3
= 945 + 3(242)
= 1671 kJ mol⁻¹
ΣδΗ(bond making) = N - Cl x 3 x 2
= 192 x 6
= 1152 kJ mol⁻¹
δHrxn = ΣδΗ(bond breaking) - ΣδΗ(bond making)
= 1671 kJ mol⁻¹ - 1152 kJ mol⁻¹
= 519 kJ mol⁻¹
they showed mandeleeves predictions were correct
Explanation:
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Assuming you meant a 0.7 mole sample of a gas, we can approximate this by assuming that the gas is acting ideally, and use the ideal gas law PV=nRT. Using the following values:
P = 1.2 Atm
V = 0.170 L
n = 0.7 mol
R = 0.08206 L-atm/mol-K
We can rewrite the equation as: PV/nR = T
Plug in our values:
(1.2 atm)(0.170 L)/(0.08206*0.7 moles) = approximately 3.55 Kelvin = T
