An unknown hot metal at 122.41°C with a mass of 53.37g was mixed with 28.15g of water at an initial temperature of 19.28°C.  A final temperature (for both water and metal) of 22.27°C was reached. In units of J/(g°C), what is the specific heat of the unknown metal?

A chemist carefully measures the amount of heat needed to raise the temperature of a  517.0mg  sample of a pure substance from  −4.5°C  to  13.7°C . The experiment shows that  2.21J  of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to  3  significant digits.

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.98 kg sample of C4H₂O from -0.4 °C to 11.4 °C. The experiment shows that 4.18 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C4H₂O? Be sure your answer has the correct number of significant digits. J-mol -1 -1 ☐ x10

An unknown substance has a mass of 25.9 g. The temperature of the substance increases from 28.7 °C to 42.9 °C when 86.4 J of heat is added to the substance. The table lists the specific heats of select substances. Substance lead silver copper iron aluminum water Specific heat [J/(g. °C)] 0.128 0.235 0.385 0.449 0.903 4.184 What is the most likely identity of the unknown substance? water silver lead copper iron aluminum