Which substance in Table 5.2 requires the smallest amount of energy to increase the temperature of 51.5g of that substance by 10K ?
All of these are specific heats of some substances at 298 K.
So N2(g) is 1.04 J/g-k
Al (s) .90 J/g-k
Fe (s) .45 J/g-k
Hg (l) .14J/g-k
H2O (l) 4.18 J/g-k
CH4 (g) 2.20 J/g-k
CO2 (g) .84 J/g-k
CaCO3 (s) .82 J/g-k

Question

Which substance in Table 5.2 requires the smallest amount of energy to increase the temperature of 51.5g of that substance by 10K ? 
All of these are specific heats of some substances at 298 K. 
So N2(g) is 1.04 J/g-k
Al (s) .90 J/g-k
Fe (s) .45 J/g-k
Hg (l) .14J/g-k
H2O (l) 4.18 J/g-k
CH4 (g) 2.20 J/g-k
CO2 (g) .84 J/g-k
CaCO3 (s) .82 J/g-k

aaronq · Answer

the one with the smallest specific heat capacity (which are the values you listed).

anonymous · Answer

Hg?

aaronq · Answer

according to your table, yes

anonymous · Answer

Okay so how do I calculate the energy needed for this temperature change.

anonymous · Answer

Cause this is all kinds of confusing to me.

anonymous · Answer

@aaronq

aaronq · Answer

Sorry, i'm not getting notifications.

you can do it in several ways, but with this information you can use the calorimetry equation:

      $q=m*C_P*\Delta T$


q= heat (energy)
Cp= specific heat capacity
m=mass
dT=change in temp

anonymous · Answer

okay sooo I'm going to walk through this and see if I get it right.

aaronq · Answer

okay, you can post it here, i'll check it out

anonymous · Answer

dT would be 298-10K right since the table is in 298K and we're figuring out for 10K?

anonymous · Answer

q= .14 J/g-k * 51.5g * 288K 
q= 2076.48

aaronq · Answer

the change in temperature is only 10 K

anonymous · Answer

oh okay

aaronq · Answer

"increase the temperature of 51.5g of that substance by 10K"

anonymous · Answer

so only 72!

anonymous · Answer

72 joules

aaronq · Answer

yep!

anonymous · Answer

Thank you!

aaronq · Answer

no problem!