The enthalpy of formation of MX is ΔHf° = –525 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 139 kJ/mol. The ionization en
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Answer:
Explanation:
Given that:
The chemical equation for the reaction is:
Br2(g) ⇌ 2Br(g)
Initially 0.0345M 0.0416M
Thus, the given reaction will proceed in the backward direction
The I.C.E table is as follows:
Br2(g) ⇌ 2Br(g)
I 0.0345 0.0416
C +x -2x
E (0.0345+x) (0.0416 -2x)
= 0.00173056 - 0.0832x - 0.0832x + 4x² = 0.00584 (0.0345 +x)
= 0.00173056 - 0.166x + 4x² = 2.0148× 10⁻⁴ + 0.00584x
= 0.00173056 - 2.0148× 10⁻⁴ - 0.166x - 0.00584x + 4x²
= 0.00152908 - 0.17184x + 4x²
Solving by using Quadratic formula
x = 0.03038 or 0.0126
For x = 0.03038
At equilibrium
[Br₂] = (0.0345 + 0.03038) = 0.06488 M
[Br] = (0.0416 -2(0.03038)) = - 0.01916 M
Since we have a negative value for [Br], we discard the value for x
For x = 0.0126
At equilibrium
[Br₂] = (0.0345 + 0.0126) = 0.0471 M
[Br] = (0.0416 -2(0.0126)) = 0.0164 M
<u>Answer:</u> The enthalpy change of the reaction is -27. kJ/mol
<u>Explanation:</u>
To calculate the mass of water, we use the equation:
Density of water = 1 g/mL
Volume of water = 25.0 mL
Putting values in above equation, we get:
To calculate the heat released by the reaction, we use the equation:
where,
q = heat released
m = Total mass = [1.25 + 25] = 26.25 g
c = heat capacity of water = 4.18 J/g°C
= change in temperature =
Putting values in above equation, we get:
To calculate the number of moles, we use the equation:
Given mass of ammonium nitrate = 1.25 g
Molar mass of ammonium nitrate = 80 g/mol
Putting values in above equation, we get:
To calculate the enthalpy change of the reaction, we use the equation:
where,
q = amount of heat released = -0.428 kJ
n = number of moles = 0.0156 moles
= enthalpy change of the reaction
Putting values in above equation, we get:
Hence, the enthalpy change of the reaction is -27. kJ/mol