Answer:

Explanation:
Hello!
In this case, since it is observed that hot cadmium is placed in cold water, we can infer that the heat released due to the cooling of cadmium is gained by the water and therefore we can write:

Thus, we insert mass, specific heat and temperatures to obtain:

In such a way, since the specific heat of cadmium and water are respectively 0.232 and 4.184 J/(g °C), we can solve for the equilibrium temperature (the final one) as shown below:

Now, we plug in to obtain:

NOTE: since the density of water is 1g/cc, we infer that 25.00 cc equals 25.00 g.
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Answer:
C
Explanation:
the enthalpy of reaction is independent of the reaction path
6.21 x 10^3 = (Move decimal point 3 spaces to the right)
6210
6210 (0.1050)
652.05
Answer:
I remember doing this in 7th,
1. D
2. B or D, more leaning on B though
3. A
To determine the heat dissipated when a substance freezes, we multiply the heat of fusion of the substance to the mass of the substance that freezes. We calculate as follows:
Heat = -3.16 (64/32.06) = - 6.32 kJ
Hope this answers the question.