How much heat is required to melt 110g of ice at-45°C?
Well, if we're talking about melting ice at -45°C, I'd say it's going to take a whole lot of heat! In fact, it's going to be colder than a penguin's freezer in there! But let's get down to the nitty-gritty. The specific heat capacity of ice is around 2.09 J/g°C, and the heat of fusion for ice is approximately 334 J/g.
First, we need to warm up the ice from -45°C to 0°C. That'll take some serious effort, but using the specific heat capacity, we can calculate the heat required for that.
Q1 = m * c * ΔT
Q1 = 110g * 2.09 J/g°C * (0°C - -45°C)
Q1 = 110g * 2.09 J/g°C * 45°C
Q1 = 10395 J
So we need 10395 J to warm up the ice to 0°C.
Next, we need to melt the ice at 0°C into water at 0°C. To do that, we use the heat of fusion.
Q2 = m * ΔHf
Q2 = 110g * 334 J/g
Q2 = 36740 J
We need 36740 J to melt the ice at 0°C.
Now we add the two amounts of heat together to get the total amount of heat required:
Total heat = Q1 + Q2
Total heat = 10395 J + 36740 J
Total heat = 47135 J
So, it'll take approximately 47135 J of heat to melt 110g of ice at -45°C. That's enough heat to make even the most frigid heart melt!
To calculate the amount of heat required to melt ice, we need to consider two processes: raising the temperature of the ice from -45°C to 0°C, and then melting the ice at 0°C.
First, we need to find out the heat required to raise the temperature of the ice from -45°C to 0°C. The specific heat capacity of ice is 2.09 J/g°C.
Q1 = m * c * ΔT
where:
Q1 = heat energy required
m = mass of ice
c = specific heat capacity of ice
ΔT = change in temperature
Plugging in the values:
Q1 = 110g * 2.09 J/g°C * (0°C - (-45°C))
Q1 = 110g * 2.09 J/g°C * 45°C
Q1 = 1086.15 J
Now, we need to calculate the heat energy required to melt the ice. The heat of fusion for ice is 333.55 J/g.
Q2 = m * ΔHfus
where:
Q2 = heat energy required
m = mass of ice
ΔHfus = heat of fusion of ice
Plugging in the values:
Q2 = 110g * 333.55 J/g
Q2 = 36690.5 J
Finally, we add the two heat energies together to get the total heat required:
Total heat required = Q1 + Q2
Total heat required = 1086.15 J + 36690.5 J
Total heat required = 37776.65 J
Therefore, it would require 37776.65 J of heat to melt 110g of ice at -45°C.
To determine the amount of heat required to melt ice, we need to use the equation:
Q = m * ΔHf
where:
Q is the amount of heat required
m is the mass of the substance being melted (in this case, ice)
ΔHf is the heat of fusion, which represents the amount of heat required to change a substance from solid to liquid at its melting point.
For ice, the heat of fusion is 334 J/g.
Now, let's calculate the amount of heat required to melt 110g of ice at -45°C:
Q = 110g * 334 J/g
Q = 36740 J
Therefore, 36740 Joules of heat are required to melt 110g of ice at -45°C.
q1 = heat need to change temperature of solid ice at -45 C to solid ice at 0 C.
q1 = mass ice x specific heat solid ice x (Tfinal-Tinitial)
q2 = heat needed to change solid ice at 0 C to liquid water at 0 C.
q2 = mass ice x heat fusion water.
Total q = q1 + q2