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An instructive illustration depicting the concept of a thermal physics experiment. Display a large block of ice at 0 degrees Celsius and a container withholding five kilograms of water at 40 degrees Celsius. Make sure to create a composition in which the water is poised to be poured onto the ice, visually conveying the process of heat exchange and melting. Do not include any text or numbers. The illustration should be detailed and done in a realistic style with a calming color scheme to make it appealing.

Five kilograms of water at 40◦C is poured on a large block of ice at 0◦C. How much(in Kg) ice melts ?

Hf = 335 kJ/kg

cw = 4.184 kJ/(kg·◦C

Sum of heats gained=0

since you know the final temp will be water at 0C, you dont have to worry about the unmelted ice. You can verify that with the solution.
heat lost by water +heatgainedbyice meleting=0
5kg*SpecHeatwater*(40-0)- MassIcemelted*335 =0

solve for massIceMelted.

2.5

80

Five kilograms of water at 40◦C? That sounds like a pretty hot tub! Careful not to jump in, though, since we're about to make some ice. Now, let's do some calculations.

To find out how much ice melts, we need to calculate the heat required to melt the ice. The heat of fusion (Hf) for ice is 335 kJ/kg. And the specific heat capacity of water (cw) is 4.184 kJ/(kg·◦C).

Since we're pouring 5 kg of water at 40◦C, we first need to cool it down to 0◦C. The heat lost by the water can be given by the equation:

Heat lost = mass × specific heat capacity × change in temperature

So, the heat lost by the water can be calculated as:

Heat lost = 5 kg × 4.184 kJ/(kg·◦C) × (40◦C - 0◦C)

After we've cooled down the water to 0◦C, we need to calculate the heat required to melt the ice. This can be given by the equation:

Heat required to melt ice = mass of ice melted × heat of fusion

Since we don't know the mass of ice melted yet, let's call it 'm'. The equation becomes:

Heat required to melt ice = m × 335 kJ/kg

Now, here's the catch: The heat lost by the water is equal to the heat required to melt the ice. So, we can set up an equation:

5 kg × 4.184 kJ/(kg·◦C) × (40◦C - 0◦C) = m × 335 kJ/kg

All we have to do now is solve this equation for 'm', and we'll have our answer! Just be careful not to melt your brain while doing the math.

To determine how much ice melts, we need to calculate the heat required to raise the temperature of the water from 40◦C to its melting point, as well as the heat required to melt the ice.

First, we find the heat required to raise the temperature of the water using the specific heat capacity of water (cw). The formula to calculate heat (Q) is:

Q = m * cw * ΔT

Where:
Q = heat
m = mass
cw = specific heat capacity of water
ΔT = change in temperature

Given:
m = 5 kg
cw = 4.184 kJ/(kg·◦C)
ΔT = (melting point of water - initial temperature of water)

Since the melting point of ice is 0◦C, we have:

ΔT = 0 - 40 = -40◦C

Now we can calculate the heat required to raise the temperature:

Q1 = m * cw * ΔT
= 5 kg * 4.184 kJ/(kg·◦C) * -40◦C

Next, we need to calculate the heat required to melt the ice. The formula to calculate heat required to melt ice (Q2) is:

Q2 = m * Hf
Where:
Q2 = heat required to melt ice
m = mass of ice
Hf = heat of fusion

Given:
Hf = 335 kJ/kg

We are pouring 5 kg of water on the ice, so the mass of ice (m) that can be melted will be equal to the mass of water poured (5 kg).

Finally, we can calculate the total heat required:

Total Heat = Q1 + Q2

Now you can substitute the calculated values into the equations to find the heat, and then determine the amount of ice melted by dividing the heat by the heat of fusion.