We’re being asked to calculate theamount of energyforced to convert36.0 g of liquid water at 65 ˚C to a gas at 115 ˚C. There are 3 heats connected in this problem:

1.

You are watching: How much energy is required to heat 40.7 g of water (h2o) from −10∘c to 70∘c?

q1which is thewarmth in raising the temperature of 36.0 g of waterfrom65 ˚C to 100 ˚C

2.q2which is thewarm in evaporating 36.0 g of waterat100˚C

3.q3which is thewarm in raising the temperature of 36.0 g of water vaporfrom100˚C to 115˚C

We should fix for each heat individually then include them together to obtain the last answer.

How much energy is forced to warmth 36.0 g H2O from a liquid at 65°C to a gas at 115°C?The adhering to physical data may be useful.

ΔHvap = 40.7 kJ/mol

Cliq = 4.18 J/g°C

Cgas = 2.01 J/g°C

Csol = 2.09 J/g°C

Tmelting = 0°C

Tboiling = 100°C

A) 52.7 kJ B) 91.7 kJ C) 87.7 kJ D) 63.5 kJ E) 10.9 kJ

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Based on our data, we think this trouble is relevant for Professor Donnelly's course at UCF.

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