1. In an experiment to determine the Specific Heat of Nickel, a 66.0 g sample of Nickel metal is heated to a temperature of 101.0 °C in a bath of boiling water. The Nickel is then removed from the Water bath and quickly added to a calorimeter containing 80.0 g of Water [C, of Water = 4.18 g °c] at an initial temperature of 23.6 °C. After thermal equilibrium was reached, the final temperature of the system was 31.1 °C. a. What is the Specific Heat of Nickel, as determined by this experiment?

The temperature of the solution increases from 21.3 °C to 38.2 °C. 0.468 g Mg reacting0.0193 mol Mg reacting80.844 g HCl solution The energy released is given by q = specific heat × mass × temperature changeThe solution is almost all water, so we use the specific heat capacity of water, 4.18 J/g•°C. What is the quantity of heat released? Enter your answer as a positive value.

q represents the change in heat of a reaction or substance. The units of q are Joules (J) or kilojoules (kJ). For a well understood substance, we can calculate the specific heat which relates the mass of the substance in grams to the amount of heat in J required to raise that amount a certain temperature.  We call that specific heat.  The specific heat (Cs) of water is stated in the following way:  C s ( H 2 O ) = 4.186 J g ∘ C This means that it takes 4.186 J of energy to raise the temperature of 1g of water by 1ºC.  The relationship between q and Cs for a given substance is  where m is mass (g) and ∆T is the change in temperature in ºC (final temp - initial temp).  Calculate the heat change (q) in J when 4.297 grams of water is cooled from 3.967 ºC to -2.902 ºC. Enter your answer with one decimal place (tenths).  Pay careful attention to the sign of your answer.  The sign of ∆T is always the same as the sign for q.

6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).