A sample of aluminum with a mass of 53.4 g is initially at 156 ∘∘ What is the temperature of the aluminum after it loses 2.75 x 103J? The specific heat capacity of aluminum is 0.903 ??∘?Jg∘C.

A 9.323 g sample of metal at 99.15 °C was placed in a calorimeter containing 35.5 g of water 19.42 °C. The temperature of the water in the calorimeter rose to 22.67 °C. What is the speci heat of the metal? (s of water is 4.184 J/(g °C))

A 735g sample of metal with a specific heat capacity of 0.282 of J/g•ºC is initially at a temperature of 21.8ºC. If 1.42 kJ of heat were added, what is the final temperature of the metal in ºC?

H8. A student combined 107.5 mL of 0.2400 M HCl and 127.9 mL of 0.3650 M NaOH in a calorimeter of negligible heat capacity . The reactants were initially at 27.1 degrees Celsius. Determine the final temperature this mixture should reach in degrees Celsius (oC), given that the heat of neutralization of this reaction is -56.2 kJ/1 mol water, the specific heat capacity of water is 4.184 J/(g.oC) and assuming that the density of all the solutions is 1.00 g/mL (Hint: The reaction between an acid and a base produces a salt and water)

15.0  J of heat is added to 10.00 g of gold, which is initially at 25°C.The heat capacity of gold is 25.41 J/(mol • °C).  What would be the final temperature of the gold?

We place a metal rod weighing 5.00 g with a specific heat capacity of 0.320 J/K/g in 20.4 mL of water. The specific heat capacity of water is 4.184 J/K/g and we make the approximation that its density is exactly 1.000 g/mL. The water has an initial temperature of 20.0 oC and the metal rod has an initial temperature of 88.0 oC. What is the final temperature (in oC) of the water and metal rod?

A bomb calorimeter has a heat capacity of 6.067 kJ/°C. A sample of vitamin (C31H4602) has an internal energy (DE) = -2.278 X 104 kJ/mol. When 1.434 g of the vitamin sample are burned in oxygen in the calorimeter, determine the final temperature in °C if the initial temperature is 14.51 °C.

Suppose that 23g of each of the following substances is initially at 25.0 ∘C∘C. What is the final temperature of each substance upon absorbing 2.30 kJ  of heat?   gold silver aluminum water

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?

a) Two substances, lead and granite, initially at different temperatures, come into contact and reach thermal equilibrium. The mass of lead is 20.4 gg and its initial temperature is 55.7 ∘C∘C. The mass of granite is 18.7 gg and its initial temperature is 22.7 ∘C∘C. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of lead is 0.128 J/(g⋅∘C)J/(g⋅∘C); the specific heat capacity of granite is 0.79 J/(g⋅∘C)J/(g⋅∘C).) b) A 4.03 gg sample of gold, initially at 70.4 ∘C∘C, is submerged into 60.8 gg of water at 17.8 ∘C∘C in an insulated container. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of gold is 0.128 J/(g⋅∘C)J/(g⋅∘C);the specific heat capacity of water is 4.18 J/(g⋅∘C)J/(g⋅∘C).)