A piece of metal weighing 10.0 g is heated to raise its temperature from 25.0 °C to 76.5 °C. It is found that the metal absorbed 47.6 cal of heat in the process.(4pts)a. Calculate the specific heat of the metal. Include appropriate units.Note that mis mass of solution in Equation 8.1.

A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celcius is added to 50.00 grams of water initially at 10.67 degrees Celcius. The final temperature of the system is 20.15 degrees Celcius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C).

n a different experiment it is observed that 252 J of heat must be absorbed to raise the temperature of 50.0 g of Ni(s) from 20.0 °C to 31.4 °C. Calculate the specific heat of Ni in both J/g·°C and cal/g·°C.

A 126-gram sample of titanium metal is heated from 20.0°C to 45.4°C while absorbing 1.68 kJ of heat. What is the specific heat of titanium? a 0.667 J/g⋅∘C b 0.294 J/g⋅∘C c 0.525 J/g⋅∘C d 0.471 J/g⋅∘C

5.25g of unknown metal at 990C was placed into 15.0 g of water at 250C. The mixture came to a final temperature of 410C. What is the specific heat of the metal if the specific heat of water is 4.184 J/g0C?Group of answer choices191 J/gºC17.3 J/gºC3.30 J/gºC-3.30 J/gºC

5.0GJ of energy is absorbed by 1.25×10 4 kg of a pure metal at its melting point. It melts and no temperature change is recorded. What is the latent heat of fusion of this metal?