The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00...
The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, the temperature of the solution decreases from 25.00 °C to 22.56 °C. Based on this observation, calculate the dissolution enthalpy, ΔdissH, of CsCl. Assume that the specific heat capacity of the solution is 4.184 J g-1 °C-1 and that the energy transfer to the calorimeter is negligible.
ΔdissH = kJ/mol
Homework Answers
Total mass of the sample = 11.9+117
= 128.9 grams
Q = mass * specific heat*∆T
= 128.9 * 4.184 * ( 25-22.6)
= 1294.36 joules
Moles of CsCl = mass / molar mass
= 11.9 / 168
= 0.071
Now, 0.071 mole absorbs 1294.36 joules
1 mole will absorb = 1294.36 / 0.071
= 18230.423 joules
Or 18.230 KJ/mol
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The salt cesium chloride is soluble in water. When 11.9 g CsCl
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The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, th...
The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, the temperature of the solution decreases from 25.00 °C to 22.56 °C. Based on this observation, calculate the dissolution enthalpy, ΔdissH, of CsCl. Assume that the specific heat capacity of the solution is 4.184 J g-1 °C-1 and that the energy transfer to the calorimeter is negligible. ΔdissH = kJ/mol
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