A 32.5 g sample of metal X require 659 J of energy to heat it from 10°C to 77°C calculate the specific heat capacity of metal X. Round your answer to significant figures. 3.35 J/g °C
0.303 J/g °C
2170 J/g °C
169 J/g °C

0.303 J/g°C.

Explanation:

From the question given above, the following data were obtained:

Mass (M) of metal = 32.5 g

Heat (Q) required = 659 J

Initial temperature (T1) = 10 °C

Final temperature (T2) = 77 °C

Specific heat capacity (C) of metal =.?

Next, we shall determine the change in temperature of the metal. This can be obtained as follow:

Initial temperature (T1) = 10 °C

Final temperature (T2) = 77 °C

Change in temperature (ΔT) =.?

Change in temperature (ΔT) = T2 – T1

Change in temperature (ΔT) = 77 – 10

Change in temperature (ΔT) = 67 °C

Finally, we shall determine the specific heat capacity of the metal as follow:

Mass (M) of metal = 32.5 g

Heat (Q) required = 659 J

Change in temperature (ΔT) = 67 °C

Specific heat capacity (C) of metal =.?

Q = MCΔT

659 = 32.5 × C × 67

659 = 2177.5 × C

Divide both side by 2177.5

C = 659/2177.5

C = 0.303 J/g°C

Therefore, the specific heat capacity of the metal is 0.303 J/g°C.

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o