How many kilocalories of heat are required to melt 20.0 kg of ice at 0°C?
Okay so the given is
m=20.0kg
Ti=0°C
HeatFusionIce=80 kcal/kg
so the setup would be
(20.0)(80)=1600cal?
right
To find the amount of heat required to melt the ice, we can use the formula:
Q = m * HeatFusionIce
Where:
Q is the amount of heat in kilocalories (kcal)
m is the mass of the ice in kilograms (kg)
HeatFusionIce is the heat of fusion for ice in kilocalories per kilogram (kcal/kg)
Given:
m = 20.0 kg
HeatFusionIce = 80 kcal/kg
Substituting the given values into the formula, we have:
Q = 20.0 kg * 80 kcal/kg
Q = 1600 kcal
Therefore, 1600 kilocalories of heat are required to melt 20.0 kg of ice at 0°C.
To calculate the number of kilocalories of heat required to melt 20.0 kg of ice at 0°C, we need to use the formula:
Heat = mass × heat fusion
where
mass (m) = 20.0 kg (given)
heat fusion (per unit mass of ice) = 80 kcal/kg (given)
Plugging in the values,
Heat = 20.0 kg × 80 kcal/kg
Now, multiply the mass and the heat fusion value:
Heat = 1600 kcal
Hence, the number of kilocalories of heat required to melt 20.0 kg of ice at 0°C is 1600 kcal.