When a 190 g piece of iron at 160 degrees celsius is placed in a 130 g aluminum calorimeter cup containing 260 g of an unknown liquid at 10 degrees celsius, the final temperature is observed to be 38 degrees celsius. what is the specific heat of the unknown liquid in calories/gram-degree-c?

0.44 cal/(g C)

Explanation:

I assume the calorimeter is adiabatic.

First I need the specific heat capacity of iron, this is:

Cp(Fe) = 0.11 cal/(g * C)

Both bodies in the calorimeter will exchange heat until they reach equilibrium at the final temperature. The heat exchanged by each body is:

Q = m * Cp * (tfin - ti)The iron will be giving off heat (negative heat) and the liquid receiving it (positive heat, so:

-m(Fe) * Cp(Fe) *(tfin - ti(Fe)) = m(liq) * Cp(liq) * (tfin - ti(liq))

Rearranging:

So:

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

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