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?

2 Answers
Thomas K.
Apr 16, 2018

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

Nam D.
Apr 17, 2018

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"

Related questions
See all questions in Specific Heat
Impact of this question
56339 views around the world
You can reuse this answer
Creative Commons License