A50.0 g sample of water at 100.00 c was placed in an insulated cup. then 25.3 g of zinc at 25.00 c was added to the water. the temperature of the water dropped to 96.68 c. what is the specific heat of the zinc ( the specific heat of h2o is 4.184 j/g c.

Taking into account the expressions and the principle of calorimetry that ensures that the body with a higher temperature will give up thermal energy to the one with a lower temperature until both are in an identical energy state, the specific heat of the zinc is 0.383 .

In first place, you need to know that the Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

The equation for calculating heat exchanges results from the product of the specific heat times the mass of the body and the temperature difference. That is, the amount of heat that a body receives or transmits is determined by:

Q = c×m×ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation (being ΔT= Tfinal - Tinitial)

On the other hand, a calorimeter is a device used to measure the heat of flow of a chemical reaction or physical change. It consists of a container built with insulating walls that limit heat exchanges with the environment in which the substances that give and receive heat are found. Being in a container with insulating walls that do not allow the exchange of energy with the outside, a principle ensures that the body with a higher temperature will give up thermal energy to the one with a lower temperature until both are in an identical energy state. That is, the heat change in the system must be 0. This is:

Qsystem= Qabsorbed  + Qyielded

0= Qabsorbed  + Qyielded

In this case, the water, when going from a higher temperature to a lower one, delivers a quantity of heat. Then

Qyielded= Qwater= cwater×mwater ×ΔT= 4.184 × 50 g× (96.68 C - 100 C)

On the other hand, the heat given off by the water will be absorbed by the zinc. Then:

Qabsorbed= Qzinc= czinc×mzinc×ΔT= czinc× 25.3 g× (96.68 C - 25 C)

Taking into account the principle mentioned above, it is possible to express:

0= czinc× 25.3 g× (96.68 C - 25 C) + 4.184 × 50 g× (96.68 C - 100 C)

Solving:

0= czinc× 25.3 g× (96.68 C - 25 C) + 4.184 × 50 g× (96.68 C - 100 C)

0= czinc× 25.3 g× 71.68 C + 4.184 × 50 g× (-3.32 C)

0= czinc× 1813.504 g×C - 694.544 J

694.544 J=  czinc× 1813.504 g×C

0.383 =czinc

In summary, the specific heat of the zinc is 0.383

Learn more about calorimeter:

8.2689J/gC

H=mc(change in temp)

H(water)=50*4.184*3.32=694.5J

H(zinc)=694.5J

c(zinc)=694.5/(25.3*3.32)=8.2689J/gC

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.