The specific heat of silver is 0.237 J/goC

Its melting point is 961oC . Its heat of fusion is 11 J/g. How much heat (in J) is needed to change 17.5 g of silver from solid at 25oC to liquid at 961oC ?

Add the heat required to warm the silver from room temp to the mp. Then add the heat to melt for the mass of silver. I will be happy to critique your work

Explain Bot Explain Bot answered
9 months ago

To calculate the total heat needed to change the silver from a solid at 25oC to a liquid at 961oC, we need to consider two steps: heating the silver from 25oC to its melting point (961oC), and then melting it.

Step 1: Heating the silver from 25oC to 961oC
To calculate the heat required to raise the temperature of the silver from room temperature (25oC) to its melting point (961oC), we will use the formula:

q = m * c * ΔT

where:
q is the heat (in Joules)
m is the mass of the silver (in grams)
c is the specific heat capacity of silver (0.237 J/goC)
ΔT is the change in temperature (961oC - 25oC)

Plugging in the values, we have:
q1 = 17.5 g * 0.237 J/goC * (961oC - 25oC)

Step 2: Melting the silver at its melting point
To calculate the heat required to melt the silver at its melting point, we will use the formula:

q = m * ΔHf

where:
q is the heat (in Joules)
m is the mass of the silver (in grams)
ΔHf is the heat of fusion of silver (11 J/g)

Plugging in the values, we have:
q2 = 17.5 g * 11 J/g

Finally, we can calculate the total heat required by adding the results from steps 1 and 2:

Total heat = q1 + q2

I will now do the calculations.