When 1.81 g of zinc metal reacts with 100.00 g of 1.00M HCl in a coffee-cup calorimeter, the temperature rises from 20.8°C to 42.3°C. The heat capacity of the calorimeter apparatus is 109 J/°C. Calculate AH (in kJ) for the reaction from the 1.81 g zinc metal: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) Assume the specific heat of the solution is 4.18 J/°C-g.

When a 8.52 g sample of solid potassium hydroxide dissolves in 123.2 g of water in a coffee-cup calorimeter, the temperature rises from 21.6°C to 29.2°C. Write a balanced equation for the reaction and calculate AH in kJ/ mol KOH for the solution process. AHrm · mol = -msolnSsolnATsoln

You mix 125 mL of 0.270 M CsOH with 50.0 mL of 0.675 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 22.30 °C before mixing to 25.42 °C after the reaction. CsOH (aq) + HF (aq) yields CsF (aq) + H2O (l) What is the enthalpy of reaction per mole of CsOH? Assume the densities of the solutions are all 1.00 g/mL, and the specific heat capacities of the solutions are 4.2 J/g · K.

A 0.600 g sample of tristearin (C57H11O6), a common fat, is combusted in a bomb calorimeter containing 750.0 g of water. The heat capacity of the calorimeter is 326 J/K.  The initial temperature is 19.5 °C. It is known that the heat of combustion of tristearin is -38.0 kJ/g. The specific heat capacity of water is 4.184 J/g.K.(a) How much heat (in kJ) is released by this reaction? (b) What is the final temperature (in °C)?

A piece of metal weighing 45.0 g was heated to 95.0oC, and the hot metal was added to 50.0 g of cold water in a Styrofoam cup calorimeter. The initial temperature of cold water was 20.0oC. If the final temperature of water and metal was 26.5oC, what is the specific heat of the metal? (The specific heat of water is 4.184 J/g.oC)           (A) 0.98 J/g.oC                           (B) 0.84 J/g.oC                           (C) 0.44 J/g.oC                           (D) 0.28 J/g.oC

150 mL of a 0.728 M HCl aqueous solution is mixed with 150 mL of 0.364 M Ba(OH)2 aqueous solution in a coffee-cup calorimeter. Both the solutions have an initial temperature of 26.5°C. Calculate the final temperature of the resulting solution, given the following information: H+(aq) + OH- (aq) → H2O(ℓ)       ΔHrxn = -56.2 kJ/mol Assume that volumes can be added, that the density of the solution is the same as that of water (1.00 g/mL), and the specific heat of the solution is the same as that for pure water, 4.184 J/(gK).

The following reaction is endothermic. 2 ZnO(s) 2 Zn(s) + O2(g) AH(1) = 697 kJ Calculate the enthalpy change for the reaction of the elements to form one mole of ZnO(s). Zn(s) + 1/2 O2(g) ZnO(s) AH(2) = kJ

When 3.12 g of glucose, CoH1206, is burned in a bomb calorimeter, the temperature of the calorimeter increases from 23.8 °C to 35.6 °C. The calorimeter contains 775 g of water, and the bomb itself has a heat capacity of 893 J/°C. How much heat was produced by the combustion of the glucose sample?

Calcium hydroxide is prepared by adding calcium oxide to water: CaO (s) + H2O (l) → Ca(OH)2 (s) Calculate the enthalpy change (ΔH) for this reaction considering the following experiment.  A 10.0 g sample of CaO (s) {MM = 56.08 g/mol} is added to 1.00 liter of water in a calorimeter with a total heat capacity of 4.37 kJ K-1 and the temperature increases by 2.70 K.

The addition of 3.15 g of Ba(OH)2∙8H2O to a solution of 1.52 g of NH4SCN in 100 g of water in a calorimeter caused the temperature to fall by 3.1 °C. Assuming the specific heat of the solution and products is 4.20 J/g °C,calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation:Ba(OH)2∙8H2O(s) + 2NH4SCN(aq) ⟶ Ba(SCN)2(aq) + 2NH3(aq) + 10H2O(l)