4.11 g of a solid (17.3 g moF') was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.2 J K. Prior to mixing everything was equilibrated to 29.1 °C. The resulting solution with a mass of 38.9 g was observed to be at a temperature of 41.7 °C and have a specific heat capacity of 4.32 J g-1 K-1. Determine g per mole for this dissolution process. Oa. -3080 J/mol Ob. 1.66 x 105 J/mol Oc. 1.30 x 104 J/mol Od. 8910 J/mol Oe. -1.30 x 104 J/mol

In a coffee cup calorimeter, a student places 0.500 g of calcium, followed by addition of 50.0 mL of 1.00 M hydrochloric acid. After the reaction took place, a temperature change of 24.7oC was observed. If the reaction solution has the same properties of water and the calorimeter constant is 5.10 J oC-1, what is the enthalpy of reaction in kJ mol-1? (Note: The mass of solution is the mass of all components added.)

22.68g of an unknown sample, with a molar mass of 53.90g/mol, reacts with excess reagents inside a simple calorimeter. The outside of the calorimeter is made of an aluminum cup with a mass of 81.0g. There is 136g of water inside the calorimeter. The temperature of the entire calorimeter increases from 20.0°C to 22.9°C. What is the molar enthalpy of reaction, in kJ/mol, with respect to the unknown?

When 35.0 mL of 0.250 M acetic acid solution, initially at 25.00oC, is added to excess dilute sodium hydroxide solution, also initially at 25.00oC, in a neutralization reaction, in a calorimeter, the temperature increases to 26.35 oC. The mass of the final solution is 85.0 g. Assuming the specific heat of the solution and products is 4.18 J/goC. Calculate the enthalpy change in kJ, Δ H, for this reaction.HC2H3O2(aq) + NaOH(aq) --> NaC2H3O3(aq) + H2O(l)

6. 100.0 mL of 1.00 M of HCl and 100.0 mL of 2.00 M of Ca(OH)2 are mixed at 298K. During the experiment, the temperature rose to 298.0067 K. Assume the heat capacities of the two solutions and densities are the same as that of water (4.184 J/g °C and 1.00 g/mL). Calculate the heat of neutralization in units of (kJ/mol H₂0 produced).

Two student chemists measured 25.0mL of 1.00 M NaOH in separate calorimeters as in the experimental procedure, Part B. Student 1 added 25.0mL of 1.10 M HCl in his solution of NaOH. Student 2 added 22.7mL of 1.10 M HCl in his NaOH solution. Each student recorded the temperature change and calculated the enthalpy of neutralization. Complete the following table to assist in answering the below questions. NOTE: Limiting reactant needs to be identified to calculate the enthalpy of neutralization. Student 1   Moles of NaOH              _________   Moles of HCl added       _________   Limiting reactant            _________   Moles of H2O produced _________   Mass of final mixture     _________     Student 2   Moles of NaOH              _________   Moles of HCl added       _________   Limiting reactant            _________   Moles of H2O produced _________   Mass of final mixture     _________     Explain why and how (higher or lower) the temperature will be different for the two…

In a calorimetry experiment similar to the one performed today, a student used 50.0 ml of 1.0 m NaOH and 5.0 ml of 1.0 m HCL each initially at 22.5ºC. The max temp observed after mixing was 28.0º C. What is the heat of reaction in units of kJ ?

4. Suppose 5 mL of 1.5 M ethylene diamine is added to 50 mL of 0.15 M Ni? solution in an identical calorimeter used in this experiment. The temperature rose 1.10°. Using the value for c of solution and C of the calorimeter, calculate AH for the formation of the ethylenediamine bonds. in kJ/mol.

7. The heat evolved from the combustion of 0.94g ethanol raises the temperature of 250 cm³ water contained in a copper beaker by 20.0 °C. [Specific heat capacity of solution = 4.18 Jg1 °C; density of solution = 1.0 g cm-3] i) What is the enthalpy of combustion per mol of ethanol? ii) Calculate the temperature rise when 1.50 g ethanol is used to heat 500 cm3 water in the same copper beaker.

In a constant-pressure calorimeter, 50.0mL of 0.340MBa(OH)2 was added to 50.0mL of 0.680MHCI. The reaction caused the temperature of the solution to rise from 23.86°C to 28.49°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). Q =