When 34.5 mL of 0.545 M H2SO4 is added to 34.5 mL of 1.09 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate H of this reaction per mole of H2SO4 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water: d = 1.00 g/mL and c = 4.184 J/g×K.)

Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer

When 28.7 mL of 0.500 M H₂SO4 is added to 28.7 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50 °C, the temperature rises to 30.17 °C. Calculate AH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the g same as for pure water.) (density for water = 1.00 .) Be sure your answer has the correct number of significant figures. mL Note: Reference the Phase change properties of pure substances table for additional information. kJ -H₂O mol

In this experiment you will place a sample of your salt in water in a constant pressure calorimeter.  You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss.   A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃  and the final temperature was 27.086365℃.   What is the number of moles of SrCl2? 4.368 g SrCl2  x  ( 1 mol SrCl2 / 123.073 g SrCl2 )  =   0.035491131 mol SrCl2   a. 0.035491 mol SrCl2 b. none of these c. 0.035 mol SrCl2 d. 0.03 mol SrCl2 e. 0.0355 mol SrCl2 f. 0.04 mol SrCl2 g. 0.035491131 mol SrCl2 h. 0.03549 mol SrCl2

Suppose 300 mL of 2.00 M HCl and 300 mL of 2.00 M NaOH, both initially at 23.0 celsius, are mixed in a thermos flask. When the reaction is complete, the temperature is 36.6 celsius. Assuming that the solutions have the same heat capacity as pure water, compute the heat released in kJ

A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.

10.00 g of Compound X with molecular formula C4H8 are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.151 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Let's use our knowledge of constant volume (bomb) calorimetry to determine the heat energy in a given food sample, say a hamburger. A typical hamburger has a serving size of 105 g and consists of approximately 20% protein (21.0 g), 33% fat (34.7 g), and 47% carbohydrate (49.3 g). Assume that the heat capacity of the bomb calorimeter is 8.39 kJ K-¹, and the increase in water temperature was 13.2 K. Q5.38 Homework Unanswered How many Calories (Cal) are in the hamburger described above? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered • 4 attempts left Submit

In a coffee cup calorimeter 2.5 grams of NaOH is added 50.00 gram of water.  The water was at 22.0oC.  The solution is stirred and mixed and the temperature of the resulting solution increases to 55.0oC.  Calculate the Q, Hrxn and the ΔHrxn kJ per mole of NaOH.  The specific heat of the solution is 4.18J/goC.

50.00 mL of 1.0 M NaOH solution at 18.0°C is mixed with 50.00 mL of 1.0 M HCI solution also at 18.00°C in a calorimeter. The mixture was allowed to react to completion and the temperature of the mixture rose to 23.60°C. Use the following information to calculate the enthalpy of the reaction. Density of the mixture is 1. lg/mL Specific heat capacity of mixture 4.18J/gK Heat capacity of calorimeter 8.65J/K (Note: Express your answer to two significant figures and do no include unit (KJ/mol) in the calculated answer).