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RSB [31]
2 years ago
15

What is the minimum mass of 25°c water required to melt all 35.1 g of ice?

Chemistry
1 answer:
inn [45]2 years ago
5 0
ΔH fusion of water is 6.0 kJ/mol
mass of ice = 35.1 g
Molecular weight of water = 18.015 g / mole
number of moles of water = 35.1 / 18.015 = 1.95 mole
amount of heat required to melt ice = moles * Δ H fusion = 1.95 x 6 =11.7 kJ
mass of water at 25°C required to get this energy to a temperature 0°C
q = m C ΔT 
11700 J = m * 4.184 * (25°- 0°)
m = 111.85 g  

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Please answer asap! worth 35 points!
Gnesinka [82]

Answer:

The enthalpy of the solution is -35.9 kJ/mol

Explanation:

<u>Step 1:</u> Data given

Mass of lithiumchloride = 3.00 grams

Volume of water = 100 mL

Change in temperature = 6.09 °C

<u>Step 2:</u> Calculate mass of water

Mass of water = 1g/mL * 100 mL = 100 grams

<u>Step 3:</u> Calculate heat

q = m*c*ΔT

with m = the mass of water = 100 grams

with c = the heat capacity = 4.184 J/g°C

with ΔT = the chgange in temperature = 6.09 °C

q = 100 grams * 4.184 J/g°C * 6.09 °C

q =2548.1 J

<u>Step 4:</u> Calculate moles lithiumchloride

Moles LiCl = mass LiCl / Molar mass LiCl

Moles LiCl = 3 grams / 42.394 g/mol

Moles LiCl = 0.071 moles

<u>Step 5:</u> Calculate enthalpy of solution

ΔH = 2548.1 J /0.071 moles

ΔH = 35888.7 J/mol = 35.9 kJ/mol (negative because it's exothermic)

The enthalpy of the solution is -35.9 kJ/mol

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