How many joules of heat are required to melt 60.5g of ice at 0 degrees C?

Oh, melting ice, always going from solid to liquid! Well, to calculate the heat required to melt the ice, we need to use the equation Q = m × ΔHf, where Q represents the heat energy, m is the mass of the ice, and ΔHf is the heat of fusion.

Now, the heat of fusion for ice is approximately 334 joules per gram. So, we can plug in the values. We have m = 60.5g and ΔHf = 334 J/g.

Q = 60.5g × 334 J/g = 20,187 joules.

So, you'll need 20,187 joules of heat to melt 60.5 grams of ice. Just make sure you don't melt too much, or else you might end up with an indoor swimming pool! And trust me, no one wants that.

To calculate the amount of heat required to melt ice, we can use the equation:

Q = m * ΔHf

Where:
Q is the heat energy required (in joules)
m is the mass of the substance (in grams)
ΔHf is the heat of fusion (in joules per gram)

The heat of fusion for ice is 334 J/g.

Substituting the given values into the equation, we get:

Q = 60.5g * 334 J/g

Q = 20,227 J

Therefore, 20,227 joules of heat are required to melt 60.5g of ice at 0 degrees C.

To calculate the amount of heat required to melt 60.5g of ice at 0 degrees Celsius, we can use the equation:

Q = m * ΔH

Where:
Q = quantity of heat (in joules)
m = mass (in grams)
ΔH = heat of fusion (in joules/gram)

First, we need to find the heat of fusion for ice, which is the amount of heat required to convert 1 gram of ice at its melting point to liquid water at the same temperature. The heat of fusion for ice is approximately 334 J/g.

Now, we can substitute the values into the equation:

Q = 60.5g * 334 J/g
Q = 20187 J

Therefore, approximately 20,187 joules of heat are required to melt 60.5g of ice at 0 degrees Celsius.

q = mass ice x deltaHfusion