If 10.6 moles of water at 35°C absorbs 12.30 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g·°C. Group of answer choices 312°C 35°C 50°C 15°C 20°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

How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.

A 325-g piece of gold at 427°C is dropped into 200.0 mL of water at 22.0°C. the specific heat of gold is 0.131 J/g°C. calculate the final temperature of the mixture. (assume no heat loss to the surroundings)

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

A 87.9 g chunk of limestone (specific heat: 0.22 J/g°C) is heated to 231.9 °C and dropped into a beaker containing 300.0 g of water (specific heat: 4.184 J/g°C) at 20.2 °C.What will be the final temperature of the system after it reaches thermal equilibrium?

What mass of water will change its temperature by 10 °C when 975 J of heat is added? The specific heat of water is 4.18 J/g 0C

A piece of silver with a mass 368 g has a heat capacity of 87.2 J/°C. What is the specific heat of silver? Group of answer choices 4.184 J/g·°C 0.385 J/g·°C 0.237 J/g·°C 0.184 J/g·°C 1.322 J/g·°C