Calculate the energy absorbed when 8.5g of ice is melted at 0 Celsius.
thank you
Water is melted so we refer to the latent heat of fusion of water.
Latent heat of fusion is 334 j/g for WATER.
So we use the heat formula:
Q=mCT
Q=8.5(334)
Q=2839J
*We don't need (T) for this equation since water is being melted.
Sure, but first I need to ask you a question: Do you know how the sun likes to melt ice? It gives it a little "heat wave"! Now, let's calculate that energy absorbed.
To calculate the energy absorbed when ice melts, we need to use the equation:
Q = m * ΔHf
where:
Q is the energy absorbed in Joules,
m is the mass of ice in grams, and
ΔHf is the heat of fusion for ice, which is 334 J/g.
So, plugging in the values:
Q = 8.5g * 334 J/g
That gives us:
Q ≈ 2849 J
So, approximately 2849 Joules of energy are absorbed when 8.5 grams of ice melts at 0 degrees Celsius. Now that's some icy business, wouldn't you agree?
To calculate the energy absorbed when 8.5g of ice is melted at 0 degrees Celsius, we need to use the specific heat capacity of ice and the heat of fusion.
1. Calculate the energy required to raise the temperature of the ice from 0°C to its melting point (0°C). This can be calculated using the formula:
Q1 = m * c * ΔT
Where:
Q1 is the energy absorbed (in Joules),
m is the mass of the ice (in grams),
c is the specific heat capacity of ice (2.09 J/g°C), and
ΔT is the change in temperature (in Celsius).
Substituting the values:
Q1 = 8.5g * 2.09 J/g°C * (0 - 0) °C
Q1 = 0 Joules
Since there is no change in temperature, no energy is absorbed in this step.
2. Calculate the energy required to melt the ice at 0°C. This can be calculated using the formula:
Q2 = m * ΔHf
Where:
Q2 is the energy absorbed (in Joules),
m is the mass of the ice (in grams), and
ΔHf is the heat of fusion (334 J/g).
Substituting the values:
Q2 = 8.5g * 334 J/g
Q2 = 2839 J
Therefore, the energy absorbed when 8.5g of ice is melted at 0 degrees Celsius is 2839 Joules.
To calculate the energy absorbed when ice is melted, we need to use the equation:
Q = m * ΔHf
Where:
Q is the energy absorbed or released (in joules)
m is the mass of the substance (in grams)
ΔHf is the heat of fusion, representing the amount of energy required to change 1 gram of a substance from a solid to a liquid at its melting point (in joules/gram)
In this case, we need to find the heat of fusion of ice. The heat of fusion of ice is known to be 333.55 J/g.
Now, we can substitute the given values into the equation:
m = 8.5g
ΔHf (heat of fusion of ice) = 333.55 J/g
Q = 8.5g * 333.55 J/g
Q = 2835.18 J
Therefore, the energy absorbed when 8.5g of ice is melted at 0 Celsius is 2835.18 Joules.