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

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).

A piece of metal at a temperature of 100 °C is dropped into an equal mass of water at atemperature of 15 °C in a container of negligible mass. The specific heat capacity of wateris four times that of the metal. What is the final temperature of the mixture

What is the heat needed to heat 150 g of water from 10.0 °C to 100 °C? (specific heat of water = 4,186 J/kg °C)

A chemist mixes 75.0 g of an unknown substance at 96.5°C with 1,150 g of water at 25.0°C. If the final temperature of the system is 37.1°C, what is the specific heat capacity of the substance? Use 4.184 J / g °C for the specific heat capacity of water.  A. 368 J / g °C  B. 13.1 J / g °C  C. 0.368 J / g °C  D. 0.0112 J / g °C

0.595 g sample of steam at 107.4∘C is condensed into a container with 5.77g of water at 16.5∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 J g⋅∘C, the specific heat of steam is 2.01 Jg⋅∘C, and Δ𝐻vap=40.7 kJ/mol.