Which of the following will affect the amount of energy it takes to change the temperature of a solid substance by 10 °C?     the specific heat capacity of the substance     the atmospheric pressure     the initial temperature of the substance     the amount (mass) of the substance you have

A hot 105.9 g lump of an unknown substance initially at 154.0 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 36.2 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. rhodium ○ graphite titanium zinc tungsten aluminum Substance Specific heat (J/(g∙°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184

If a 50.0 g piece of brass rod at 98.0°C is placed in 150.0 g of water at 25.0°C, what is the final temperature? Assume that no heat is transferred to the surroundings. The specific heat capacity of water is 4.18 J/g °C. The specific heat capacity of brass is 0.38 J/g °C. 35 79 42 27

A chemist carefully measures the amount of heat needed to raise the temperature of a 286.0 g sample of a pure substance from 6.3 °C to 23.4 °C. The experiment shows that 11.9 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits. - ·K

How much heat must be added to a 38-g sample of aluminum to increase its temperature by 250.0°C? The specific heat capacity for aluminum is 0.902 J/g°C.

A hot 122.8 g lump of an unknown substance initially at 154.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 56.9 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. graphite zinc aluminum titanium tungsten rhodium Substance Specific heat (J/(g-°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 0.132 0.388 4.184 tungsten zinc water

How many calories of energy would be required to heat 120.0 grams of pure silicon dioxide (glass) from 23.50 °C to 100.0 °C given that the specific heat capacity of glass is 0.7520 J/g °C.

4. Determine the final temperature of water if 9.2 kJ of heat is added to 250 mL of 17°C water (the specific heat capacity of water is 4.184 J/g°C).

A metal object with mass of 21.4 g is heated to 97.0 °C and then transferred to an insulated container containing 81.7 g of water at 20.5°C. The water temperature rises and the temperature of the metal object falls until they both reach the same final temperature of 23.1 °C. What is the specific heat of this metal object? Assume that all the heat lost by the metal object is absorbed by the water. cal specific heat: