A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume no heat is lost to the calorimeter. C(H₂O) = 4.18 J/(g.K), C(Ni) = 0.444 J/(g.K)

To treat a burn on his hand, a person decides to place an ice cube on the burned skin. The mass of the ice cube is 12.7 g,12.7 g, and its initial temperature is −14.4 ∘C.−14.4⁢ ∘C. The water resulting from the melted ice reaches the temperature of his skin, 29.8 ∘C.29.8⁢ ∘C. How much heat is absorbed by the ice cube and resulting water? Assume that all of the water remains in the hand. q= J

A piece of titanium metal with a mass of 21.6 g is heated in boiling water to 99.5 °C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.8 °C. When thermal equilibrium is reached, the final temperature is 24.5 °C. Calculate the specific heat capacity of titanium. (The specific heat capacity of liquid water is 4.184 J/g. K.) Specific heat capacity= J/g. K

A calorimeter contained 79.0 g of water at 15.91°C. A 105-g sample of iron at 65.26°C was placed in it, giving a final temperature of 18.88°C for the system. Calculate the heat capacity of the calorimeter. Specific heats are 4.184 J/g-°C for H2O and 0.444 J/g-°C for Fe. Heat capacity of the calorimeter =| J/°C

The temperature of a sample of iron increased by 22.0 °C22.0 °C when 269 J269 J of heat was applied. What is the mass of the sample?   Substance Specific heat J/(g · °C) lead 0.128 silver 0.235 copper 0.385 iron 0.449 aluminum 0.903

You wish to heat water to make coffee. How much heat (in joules) must be used to raise the temperature of 0.120 kg of tap water (enough for one cup of coffee) from 22°C to 96°C (near the ideal brewing temperature)? Assume the specific heat is that of pure water, 4.18 J/(g.°C). Heat = J

A 6.55 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. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic?   how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius