rom −5.2°C to 19.2°C. The experiment shows that 404.J 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 119.0g sample of a pure substance from −5.2°C to 19.2°C. The experiment shows that 404.J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits.

The equation below can be used to find the specific heat capacity of a substance. Work out the specific heat capacity of a substance if it takes 5,200J of energy to heat 2kg of it from 42°C to 47°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

Calculate the energy required to heat 586.0g of mercury from 3.2°C to 19.2°C. Assume the specific heat capacity of mercury under these conditions is ·0.139J·g−1K−1 . Be sure your answer has the correct number of significant digits.

The specific heat capacity of a pure substance can be found by dividing the heat needed to change the temperature of a sample of the substance by the mass of the sample and by the change in temperature. The heat capacity of a certain substance has been measured to be 1.50J·g°C. Suppose 203.g of the substance are heated until the temperature of the sample has changed by 27.2°C.Write an equation that will let you calculate the heat Q that was needed for this temperature change. Your equation should contain only symbols. Be sure you define each symbol.