00:01
To calculate the total heat required in joules to change 6 .2 grams of silver, from a solid at 25 degrees celsius to a liquid at its melting point of 962, there are two steps involved.
00:15
First, we need to warm the silver to its melting point.
00:22
To do that, we'll use the equation q is equal to sm delta t, where s is the specific heat of silver, 0 .2 .2.
00:33
35 joules per gram degree celsius or kelvin multiplied by its mass.
00:43
The mass is 6 .20 grams multiplied by its change in temperature.
00:50
We need to warm it up to 962 from an initial temperature of 25 degrees celsius and we get 1 ,365 joules and then the second step is to melt the silver.
01:10
To melt the silver, the heat will be equal to the mass of the silver, 6 .20 grams, converted to moles using the molar mass of silver, which is 107 .87 grams in one mole silver.
01:27
And then we can use the delta h of fusion for silver, which is 11 .8 .7 grams in one mole silver.
01:32
And then we can use the delta h of fusion for silver, which is 11, 1 .3 kilojoules per mole...