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.


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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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What clinical concept do you need to understand in order to deal with this problem?

Our tutors have actually suggested that to settle this trouble you will should use the Heating and also Cooling Curves principle. You can watch video lessons to learn Heating and Cooling Curves. Or if you require even more Heating and Cooling Curves practice, you deserve to likewise practice Heating and also Cooling Curves practice difficulties.


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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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