Question 22 of 30 How much heat, in kJ, will be absorbed by a 25.0 g piece of aluminum (specific heat = 0.930 J/g-°C) as it changes temperature from 25.0 °C to 76.0 °C?

Please help me complete this question

A material has a specific heat of 0.625 J/g°C.  A 75.6 g sample of this material is heated  and them placed in 35.2 g of water at 21.4 °C.  The temperature of the water rises to 32.7 °C.  What was the initial temperature of the material?

Ethyl alcohol, C2H5OH, has a specific heat of 2.40 ?? °?. Which of the following statements best describes what this means? a) It takes 1 joule of energy to increase the temperature of 1 gram of ethyl alcohol by 2.40 °C. b) It takes 1 joule of energy to increase the temperature of 2.40 grams of ethyl alcohol by 1 °C. c) It takes 2.40 joules of energy to increase the temperature of 1 gram of ethyl alcohol by 1 °C. d) It takes 2.40 joules of energy to increase the temperature of 2.40 grams of ethyl alcohol by 1 °C

4. 30.0 g of a substance (molar mass: 46 g/mo) required 262 J of heat to raise its temperature from 32.0°C to 37.4°C. What is the specific heat per gram and per mole of this substance?

When a 0.740-g sample of trinitrotoluene (TNT), C,H,N,O, is burned in a bomb calorimeter, the temperature increases from 23.4 °C to 26.9 °C. The heat capacity of the calorimeter and its content is 3.35 kJ/°C. How much heat was produced by the combustion of the TNT sample? O 34.2 kJ O 11.7 kJ O 101.5 kJ

A sample of aluminum, initially at 5.0 °C, was placed in 18.0 g of water, initially at 25.0 °C. The final temperature of the water and the metal was 21.0 °C. The specific heat of water is 4.184 J g-1 °c-1 and aluminum is 0.940 J g-1 °C-1. Ignore the heat capacity of the container. What is the mass (in g) of the aluminum?

When a sample of titanium was supplied 1.00 kJ of energy, the temperature rose 103.5 °C. If the specific heat of titanium is 0.523 J/g · °C, what is the mass of the titanium sample?

How much heat energy (J) is given off in a reaction when 2.30g of metal (specific heat = 0.128J/g°C) experiences a temperature decrease from 100.00°C to 28.00°C, when added to water? O -72.0 J O 29.4 J O -21.2 J O 24.3 J 2

3. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal.