Question

The molar heat capacity of silver is 25.35 J/mol*C. How much energy would it take to raise the temperature of 10.2 g of silver by 14.0 degrees C?

Answer 1

`33.6J`

Explanation:

You have to use `q=mCΔT`
`m=10.2g`
`C=25.35` (J/mol)*C
`T=14C`
First convert `10.2` to moles by dividing it by the molar mass of silver
`10.2/107.8682=.0945598425`
Than plug into equation
`q=(.0945598425mol)(25.35)(14)`
`q=33.6J`

Answer 2

Around `33.6` joules

Explanation:

We use the specific heat equation, which states that,

`q=mcDeltaT`

• `m` is the mass of the object

• `c` is the specific heat capacity of the object

• `DeltaT` is the change in temperature

We got: `m=10.2 \ "g", c=(25.35 \ "J")/("mol" \ ""^@"C"),DeltaT=14""^@"C"`.

So, let's first convert that amount of silver into moles.

Silver has a molar mass of `107.8682 \ "g/mol"`. So here, we got:

`(10.2color(red)cancelcolor(black)"g")/(107.8682color(red)cancelcolor(black)"g""/mol")=0.0945598425 \ "mol"`

I will keep this number and I'll round off at the end.

So, the heat needed is:

`q=0.0945598425color(red)cancelcolor(black)"mol"*(25.35 \ "J")/(color(red)cancelcolor(black)"mol"color(red)cancelcolor(black)(""^@"C"))*14color(red)cancelcolor(black)(""^@"C")`

`~~33.6 \ "J"`