3. In this experiment, we have used 1.0 x 1.01 J/°C for the heat capacity of the coffee-cup calorimeter. Let us verify this number through the following experiment using only hot and cold water. Experimental procedure: Place 50 mL of water at 20.0 °C in the coffee cup calorimeter. i. ii. Add 50 mL of hot water at 98.0 °C to the calorimeter holding the cold water. ii. The Trof 58.0 °C was obtained through the temperature-time graph. Calculate the specific heat of the coffee cup calorimeter. Remember that the heat lost by the hot water was gained by the cold water as well as the calorimeter.

3. In this experiment, we have used 1.0 x 1.01 J/°C for the heat capacity of the coffee-cup calorimeter. Let us verify this number through the following experiment using only hot and cold water. Experimental procedure: Place 50 mL of water at 20.0 °C in the coffee cup calorimeter. i. ii. Add 50 mL of hot water at 98.0 °C to the calorimeter holding the cold water. ii. The Trof 58.0 °C was obtained through the temperature-time graph. Calculate the specific heat of the coffee cup calorimeter. Remember that the heat lost by the hot water was gained by the cold water as well as the calorimeter.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student mixed 50.0 mL of water containing 0.010 moles of HCI (weighing 50.0 g) with 60.0 mL of water containing 0.012 moles of NaOH (weighing 60.0 g) in a coffee cup calorimeter. Both solutions were initially at 25.00°C, but after reaction upon mixing the temperature rose to 26.20°C. The specific heat of the solution is the same as that of water, 4.18 J/g °C, and the calorimeter has a heat capacity of 35 J/°C. The reaction is shown below. (a) How much heat is produced in the reaction? (b) How much heat is produced if one mole of water is formed in this chemical reaction? HCl(aq) + NaOH(aq) → NaCl(aq) + H20(l)
2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
CHAPTER 5 - PRINCIPLES OF CHEMICAL REACTIVITY: EN Previous Page 3 of 5 endothermic ✓ exothermic When 1 mole of I2 (g) reacts with Cl₂ (g) to form ICI(g) according to the following equation, 26.8 kJ of energy are evolved. 1₂ (9) + Cl₂ (9) → 21C1(g) What is the value of q? kJ NOV 11 Next → othermic or exothermic? #tv ♫ P 100 Use the References to access DO Cengage Learning | C MacB
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01. The enthalpy change in a reaction is 1366 kJ per mole. Should the enthalpy of the combustion reaction be positive or negative? Explain. a. Calculate the total energy change when 14.50 grams of carbon dioxide is produced.
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
2. A student collect experimental results and show all calculation steps including units. Keep the correet significant figures. Part 1: Calculation of the calorimeter constant (15 pts) Mass of Mass of Temperature of cold water in calorimeter cold water hot water Temperature of hot water before mixing 57.3°C Final temperature of the water after mixing 36.8°C 61.0 g 56.2 g 22.6 °C Show calculations below. Part II: Conduct Reaction 1 between solutions of NaOH and HCI (20 pts) Volume of Volume of Density of the NaOH HCI Initial temperature of the solution in the calorimeter solution solution. solution 51.0 mL 52.0 mL 1.04 g/mL 22.6 °C Show calculations below. Final temperature of the reaction mixture 32.2 °C The calorimeter constant is: Enthalpy of the reaction, in kJ/mol, is
3. Suppose the 25.0 g of the following substances all initially at 27.0 °C absorb 2.35 kJ of energy. What is the final temperature of each? D) Water. You will need to look up specific heat values.
Determine the enthalpy change when 150g of 10˚C water was placed into a calorimeter. 4.90g of sulfuric acid was added and the solution rose to 14.9˚C The specific heat capacity of the solution is 4.2 J/g ˚C
1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. = 7.52 g = 7.20 g Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water Final temperature of water = 140.0 g = 10.0°C = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.