A piece of metal weighing 8.00 g  at a temperature of 46.0 oCo was placed in a calorimeter in 38.10 mL  of water at 24.3 oC. The final equilibrium temperature was found to be 25.7 oC . What is the specific heat of the metal?

Consider an unknown metal X with a mass of 67.5 g at an initial temperature of 76.1 °C. The metal is placed in 88.7 g of water initially at 20.5 °C in an insulated container. The final equilibrium temperature of the system is 32.1 °C. Calculate the specific heat (J/(g·°C)) of the metal X.   Use Cs = 4.18 J/(g·°C) for the specific heat of water. Assume that the only energy exchange that occurs is between the metal and the water.

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.   In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C.   The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C.   Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data.   Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol).   C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy

A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.

a group of chem students was asked to determine the heat of reaction for the neutralization of a newly synthesized monoprotic acid HX and NaOH. they first calibrated the styro ball calorimeter using the reaction of 15.0mL of 0.100M HCl and 20.0mL of 0.0500M KOH. this recorded a change in temperature from 26.5 °C to 31.8 °C. afterwards, they determined the heat of reaction for a mixture of 5.00mL, 1.00M NaOH and 10.0mL, 1.00M HX. this showed an increase in temperature of 3.6 °C C. What is the experimental enthalpy (in kJ/mol) for the neutralization reaction between HX and NaOH?D. Is the reaction between NaOH and HX endothermic or exothermic?

the molar heat capacity of iron is 25.10 J mol –1 K–1 . A 25.0 g ball is heated until it is glowing red (to a temperature of 400.°C). It is dropped into a 50.0 mL container of water at 25.0°C. If the density of water is 0.997 g mL–1 , and the molar heat capacity of water is 4.186 J g–1 K–1 , what temperature (in K) will the ball and water equilibrate to? A) 338 B) 300 C) 317 D) 359 E) 342

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

When a 45.0 g sample of an alloy at 100.0 °C is dropped into 55.0 g of water at 25.0 °C, the final temperature is 30.4 °C. What is the specific heat of the alloy? The specific heat of H2O(l) is 4.184 J·g–1·°C–1.            (A) 0.397 J·g–1·°C–1.           (B) 0.447 J·g–1·°C–1.           (C) 1.28 J·g–1·°C–1.           (D) 1.55 J·g–1·°C–1.

A 0.692 g sample of glucose (C6H1206) is burned in a bomb calorimeter. The temperature of 575g of water in the calorimeter rises from 21.70 °C to 25.22 °C. If the heat capacity of the bomb is 650 J.Kl and the heat capacity of the water is 4.184 J/gK-1, calculate the heat evolved per 0.692 g of glucose.

A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC