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:
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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