In a coffee cup calorimeter, 44.0 mL of 0.11 M nitric acid (HNO3) and 44.0 mL of 0.11 M potassium hydroxide (KOH) are mixed to observe the heat released during the neutralization reaction. Based on the data in the table, what is the enthalpy of the neutralization reaction between HNO3 and KOH? AHrxn= Initial temperature in the calorimeter (°C) Final temperature in the calorimeter (°C) Final mass of the neutralized solution (g) Calorimeter constant (J/°C)) 19.1 19.8 87.71 4.75 kJ/mol

In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.

In a coffee cup calorimeter, 40.0 mL of 0.33 M nitric acid (HNO3) and 40.0 mL of 0.33 M potassium hydroxide (KOH) are mixed to observe the heat released during the neutralization reaction. Based on the data in the table, what is the enthalpy of the neutralization reaction between HNO3 and KOH? Initial temperature in the calorimeter (°C) Final temperature in the calorimeter (°C) Final mass of the neutralized solution (g) Calorimeter constant (J/C)) 21.3 23.5 79.74 4.57

100.0 ml of 0.115 m potassium hydroxide solution is mixed with 75.0 ml of 0.245 M nitric acid solution in a coffee cup calorimeter. Before mixing, both solutions are initially at 23.85 C;after mixing, the temperature of the mixture in the coffee cup calorimeter increases to 26.30 C. Determine the enthalpy change(delta h) of reaction in kJ/mol for the reaction as written below. KOH(aq) + HNO3(aq) ⮕ KNO3(aq) + H2O(aq) Assume the  resulting  solution density is 1.03 g/mL. Specific heat of solution=4.20 J/g C

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?

Determine the enthalpy of reaction (DHxn) in kJ/ mol H20 formed if an acid/base neutralization if 13.6 mL of 1.205 M NaOH is reacted with 25.0 mL of 1.108 M HCI causing an increase in the calorimeter temperature of 6.85 °C. Use 3.93 J/g°C for the specific heat capacity of the final solution and the density for the final solution is 1.02 g/mL.

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?

In a coffee-cup calorimeter, 120.0 mL of 1.4 M  NaOH  and 120.0 mL of 1.4 M HCL  are mixed. Both solutions were originally at 20.6°C. After the reaction, the final temperature is 30.0°C. Assuming that all the solutions have a density of 1.0  and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCL  by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH =  kJ/mol

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.

In a constant pressure coffee-cup calorimeter, 100.0 mL of 0. 050 M of Ag+ was mixed with 100.0 ml of 0.050 M of Cl‒. The temperature changed from 298.5 K to 299.4 K. Calculate the enthalpy of reaction, ΔH (kJ/mol). Assume that the solutions have a density of water (1 g/mL) and specific heat capacity of water (4.184 J/g °C).                                        Ag+(aq) + Cl‒(aq) ⟶ AgCl(s)