A student mixes 20 mL of 0.1 M HCl and 20 mL of 0.1 M KOH in a coffee cup calorimeter. Upon complete mixing, the temperature of the resulting solution changes from 28C to 32.5C. Calculate the molar heat of reaction or neutralization

To measure the enthalpy of an acid-base reaction, a student places the thermometer in the hydrochloric acid solution, and then, without rinsing with DI water, places it in the sodium hydroxide solution prior to adding the hydrochloric acid solution to the calorimeter.  How would this affect the calculated enthalpy of the reaction, be too high, too low, or unaffected?  Why?

A 10.7 ml sample of 0.947 M NaOH is mixed with 15.9 mL of 0.955 M HOCI in a coffee-cup calorimeter. The enthalpy of the reaction, written with the lowest whole-number coefficients, is -55.8 kJ. Both solutions are at 23.0°C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, the specific heat of all solutions is the same as that of water, and volumes are additive. The specific heat of water is 4.18 J/(g °C). Temperature =

A quantity of 85.0 mL of 0.600 M HCl is mixed with 85.0 mL of 0.600 M KOH in a constant-pressure  calorimeter. The initial temperature of both solutions is  the same at 17.35°C, and the final temperature of the  mixed solution is 19.02°C. What is the heat capacity of  the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is −56.2 kJ/mol.

A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?

100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?

4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).

25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.

1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg²+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.

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