In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH)₂ was added to 70.0 mL of 0.600 M HC1. The reaction caused the temperature of the solution to rise from 23.98 °C to 28.07 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. ΔΗ = 2.396 Incorrect kJ/mol H₂O

E In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH), was added to 70.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 23.98 °C to 28.07 °C. If the solution has the same density and BO specific heat as water (1.00 g/mL and 4.184J/g °C,) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH = kJ/mol H₂O

7. In a calorimeter, 50.00 mL of 2.50 M NaOH was combined with 50.00 mL of 2.25 M HCI to form a solution. The temperature of the solution went from 20.0 °C to 36.0 °C. The heat capacity of the solution is 4.184 J/g°C. Assume a density of 1.00 g/mL Determine the AHneutzn of HCI.

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A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol

A 1.200 g sample of ZnCO3 (s) dissolved in 40.0 mL of a dilute HCl solution (density = 1.10 g/mL) in a coffee cup calorimeter, producing CO2 (g), liquid water and ZnCl2 (aq).  The temperature of the solution changes from 24.32 oC to 25.49 oC.  The resulting solution has a specific heat of 4.18 J/goC. What would be the # of heat released by the reaction and Is the reaction endothermic?

Determine the enthalpy of reaction (DH,) in kJ/ mol H,O formed if an acid/base neutralization if 11 ml of 1.205 M NaOH is reacted with 25.0 ml of 1.108 M HCI ard 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. ctor

A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs

In a constant‑pressure calorimeter, 55.0 mL of 0.340 M Ba(OH)2 was added to 55.0 mL of 0.680 HCl. The reaction caused the temperature of the solution to rise from 23.90 ∘C to 28.53 ∘C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ).