In the following experiment, solid CaCl2 is dissolved in water: CaCl2(s) → Ca2+(aq) + 2Cl-(aq)     ΔsolnH = −82.8 kJ mol−1 A coffee-cup calorimeter containing 145 mL of H2O is used. The initial temperature of water in the calorimeter is 18.9°C. If 3.04 g of CaCl2 is added to the water, what will be the final temperature of the solution in the calorimeter?  Assume the density and specific heat capacity of the solution is the same as water (d=1 g/mL, Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.

When 4.81 g of a solid mixture composed of NH4Cl and CaCl2 was dissolved in 100.0 mL of water, the temperature of the water rose by 4.44°C. How many grams of each substance was in the mixture?Include the mass of salts in calculation of heat generated.g NH4Cl =  g CaCl2 =

A 50.0 mL sample of a 1.00 MM solution of CuSO4CuSO4 is mixed with 50.0 mL of 2.00 MM KOHKOH in a calorimeter. The temperature of both solutions was 24.6 oCoC  before mixing and 32.8 oCoC  after mixing. The heat capacity of the calorimeter is 12.1 J/K.  From these data, calculate ΔHΔH for the process: CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.

In a laboratory investigation into the neutralization reaction;   HNO3 (aq) + NaOH(s) → NaNO3 (aq) + H2O (l)   a researcher adds 5.3 g of solid sodium hydroxide to 200.0 mL of 1.0 M nitric acid solution in a polystyrene calorimeter. The temperature changes from 21.0°C to 28.5°C. Calculate the molar enthalpy of neutralization of sodium hydroxide.

The reaction of zinc with hydrochloric acid is represented by the reactionZn(s) + 2 HCl(aq) ↔ ZnCl 2(aq) + H 2(g) -- ΔH = -152.5 kJ How many grams of zinc reacted with an excess of HCl (100.0 mL) if the temperature of the calorimeter increased from 25.0°C to 35.85 °C? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.

You mix 125 mL of 0.250 M CSOH with 50.0 mL of 0.625 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.70 °C before mixing to 24.59 °C after the reaction. CsOH(aq) + HF (aq) → 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. Enthalpy of reaction = kJ/mol

In an experiment, a 0.5002 g sample of tridecanedioic acid ( C13 H24 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.165 × 10³ g of water. During the combustion the temperature increases from 21.99 to 24.52 °C. The heat capacity of water is 4.184 J·g¯¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 904.0 J. °C¯¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of tridecanedioic acid based on these data. C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + Energy kJ/mol Molar Heat of Combustion =

A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 302(g) →2 KClO3(s) AH=78. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction ΔΗ ㅁ x10 2K C103 (s) → 2KC1(s) + 302(g) KCIO, (s)-KCI(s) + 0,(s) 3 KCI(s)+0, (g)KCIO, (s) kJ kJ 1 5

Which of the reactions are exothermic?

In a constant‑pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2 was added to 60.0 mL of 0.640 M HCl.The reaction caused the temperature of the solution to rise from 24.50 ∘C to 28.86 ∘C. If the solution has the same density and specific heat as water (1.00 g/mLand 4.184J/g⋅°C, respectively), what is ΔH for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes. ΔH= _________ kJ/mol H2O