(adsbygoogle = window.adsbygoogle || []).push({}); A 330-g glass mug at 16C is filled with 275 milliliters of water at 91C. Assuming no losses to the external environment, what is the final temperature of the mug?

Im having a bit of trouble with this problem. Since we're assuming no losses, delta q=0.

So, delta q= delta q(mug) + delta q (water) = 0

and delta q(mug) = mass(mug)*specific heat(mug)*delta T(mug)

and delta q(water) = mass(water) *specific heat(water)*delta T(mug)

so put it all together and i get

0=.330kg*840J/kgK*delta T(mug) + .275kg*4186J/kgK*delta T(water)

But where do i go from here? Is the change in temperature for botht he mug and the water going to be the same? in which case i could factor out a delta T, but then that still leaves me stuck.

Does the change in temperature of the water even matter at all?

Theres got to be a way to do this that im not seeing...

Thanks

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# Homework Help: Thermal dynamics

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