4. Determine the final temperature of the solution formed when 0.37 g of potassium chloride isdissolved in 100 ml of water in a calorimeter. Assume that the volume of the resulting solutionis 100 ml. The temperature before reaction is 20°C. The heat capacity of the calorimeter is10J/°C. Assume that the specific heat and density of the solution are the same as those of water.Write down all the reaction equations needed to solve this exercise. (10pts)

Step 1:To determine the final temperature of a solution when dissolving 20 g of potassium chloride…

Answered: 4. Determine the final temperature of…

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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In a simple calorimeter, a piece of metal weighing 48.67 g was heated to 120.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. Is this process endothermic or exothermic? Explain. Show Your Work
48.2 mL of a solution of HCl is combined with 110.7 mL of 1.35 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C, and the final temperature after reaction is 29.3°C. What is the molarity of the HCl solution? You may assume that there is an excess of base (so that all the HCI has reacted), that the specific heat of the reaction mixture is 0.96 cal/g °C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mole.
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
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 quantity in moles of the unknown salt were used in the reaction?
3
6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).
Please help me complete this question
Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter. The initial temperature of the water is 21.2 oC. The final temperature of the solution is 15.4 oC. The calorimeter constant = 25.2 J/oC. Is the following statement true or false? This process is exothermic. True False
3
You have 8.99 g sample of an unknown salt (MM = 116.82 g/mol). It 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 Mass inside calorimeter (g)? Change in Temp inside calorimeter (C)? How much Heat gained (J)? Total Heat? How many mols of the unknown salt? What is the change in empalthy?
The answer is 44.8 kJ/mol. Show the solution how to get 44.8 kJ/mol.
When 25.0 g hydrogen gas react according to the following reaction, how many kJ of heat are released or consumed? CO (g) + 3 H2 (g) --> CH4 (g) + H2O (g) Delta Hrxn = – 206 kJ a. – 1.28 x 103 J b. – 25.5 J c. – 639 J d. – 2.55 x 103 J e. – 1.29 x 103 J f. none of these

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