A calorimetry experiment was done on a mystery piece of metal and the data was recorded in the table below. Measurement Mass of the metal Initial temperature of the metal 89.20 g 98.1 °C Mass of the water Initial temperature of the water Final temperature of the water 47.50 g 22.5 °C 28.2 °C What was the specific heat of the mystery metal? (CH20 = 4.181 J/g°C )

A piece of metal weighing 146.7 g was heated from 32.0 °C to 56.2 °C. If the amount of heat needed was 1363.3 J, calculate the specific heat of the metal. What is the identity of the metal? 20 Specific Heats of Selected Metals Smetal, J/g-°C Metal 0.901 Smetal, J/g-°C 0.449 Metal Al Fe Cu 0.384 Ni 0.444 Si 0.711 Sn 0.226 Zn 0.389 Mn 1.02

When a  brass black was dropped into a 124-gram water, the water temperature increased from 21.0°C to 36.8°C. What is the heat capacity of the brass block? The initial temperature of the brass was 314.2°C and the specific heat of water is 4.184J/gk. If the mass of the brass block is 77.764g, what is the specific heat of the brass?

A 35.0 gram object has a specific heat of 0.832 Joules/gram °C. It gained 2095 Joules of heat from the surroundings. If it had started at 25.0 °C, what was the temperature of the object after it gained the heat from the surroundings? O 25.0 degrees Celsius O 3640 degrees Celsius O 71.9 degrees Celsius O 196.9 degrees Celsius O 1.74 degrees Celsius O 53.1 degrees Celsius O 96.9 degrees Celsius

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.55 kg sample of a pure substance from 7.7 °C to 14.6 °C. The experiment shows that 5.5 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. DJ-g`1 - K-1 ☐ x10 X

A 146.3g piece of iron (specific heat = 0.449 J/g°C) is heated with a flame and dropped into a coffe cup calorimeter containing 450.0 g of water. the water (specific heat = 4.18 J/g°C) in the calorimeter increases from 20.3°C to 32.0°C. what was the initial temperature of iron?

Expressing amounts of energy in different energy units is necessary to solve many chemistry problems. For practice, complete the following table. The Joule (J) is the SI unit of energy. 1 calorie (cal) = 4.184 J J cal kJ 549       197       0.806

A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C.   If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt?   How many moles of the unknown salt were used in the reaction ?     _______ J?

A chemist carefully measures the amount of heat needed to raise the temperature of a 149.0 mg sample of a pure substance from 13.7 °C to 31.8 °C. The experiment shows that 4.99 J 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. -1 Jg¹.K -1 0 X S