1. What is the essence of detemining the heat capacity of the calorimeter? Is it possible to replace the calorimeter in the middle of the experiment, say you use same type of calorimeter, but you borrowed from another group to perform part C and D? Why? 2. Explain the temperature profiles of the contents of the calorimeter. 3. What is the relationship of the temperature with the calculated AH? Compare the AH of the three reactions.

1. What is the essence of detemining the heat capacity of the calorimeter? Is it possible to replace the calorimeter in the middle of the experiment, say you use same type of calorimeter, but you borrowed from another group to perform part C and D? Why? 2. Explain the temperature profiles of the contents of the calorimeter. 3. What is the relationship of the temperature with the calculated AH? Compare the AH of the three reactions.

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...

See similar textbooks

Similar questions

9. A 40.0 kg industrial calorimeter has an overall specific heat capacity of 1.00 J/ (g°C). Complete combustion of 1.00 g of hydrogen in this calorimeter causes a temperature increase of 3.54°C. Calculate the molar enthalpy of combustion for hydrogen from this evidence. (-286 kJ/mol)
O 26 of 42 Constants Periodic Table Calorimetry is a method used to measure enthalpy, or heat, changes that occur during chemical processes. Two common calorimeters are constant-pressure calorimeters and constant- volume (or "bomb") calorimeters. Part A A simple constant-pressure calorimeter can be made from a foam coffee cup and a thermometer; energy changes in a reaction are observed via a temperature change of the solution in the cup. Bomb calorimeters are used to measure A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 107 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24,70 C. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures. combustion and other…
In three to five sentences. answer the following auestions. 1. Why is it necessary to indicate the physical state of all reactants and products when giving the enthalpy change for a reaction? 2. The reaction of nitrogen gas and oxygen gas to form nitrogen monoxide, NO, is favored at high temperatures. Thus, NO is found in the exhaust gases of high compression automobile engines since they operate ta high temperatures. Is the reaction endothermic or exothermic? Explain.
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Water Thermometer Metal sample 2003 Thomson-Brooks/Cole Stirring rod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 100.00 grams of nickel to 98.10 °C and then drops it into a cup containing 79.36 grams of water at 23.62 °C. She measures the final temperature to be 32.36 °C. Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant. Calorimeter Constant = J/°C
2. When a 0.0157 g of a compound with a heat of combustion of -37.6 kJ/ mole is burned in a calorimeter, 18.5 J of heat is removed. What is the MW of the compound? (provide the given and required to find in the problem) (Kindly provide a CLEAR and COMPLETE solution) (Answer should be typewritten)
20. In a chemical reaction, the amount of energy gained by the surroundings must equal the amount of energy released by the reaction(system). A. True B. False ount of heat needed to increase the temperature of one mole of a
1. In the laboratory of an educational institution there is a calorimeter like the one shown in the figure. The masses of the water and of block A are equal. Block A is placed in the calorimeter at a temperature higher than that of water. The heat transfer is carried out from: A. Block towards the water B. Water to the block C. Water to the outside environment D. Environment outside the water. 2. Taking into account question 1. The heat transfer is carried out from: A. Half of the water B. Same as water C. Double that of water D. Null 3. The attached graph shows the increase in temperature with the absorbed heat of an unknown substance. The boiling temperature of this substance is: A. T1 B. T2 C. T3 D. T4
When using a coffee cup calorimeter to determine the specific heat of a metal sample errors can occur in the procedure. Which of the following procedural errors would lead to a specific heat value being calculated that is lower than the accepted value? Check all that apply. When the metal was placed into the coffee cup calorimeter some water splashed out of the cup. After the metal was heated (to its initial temperature) there was a significant time delay before it was placed into the coffee cup calorimeter. After the mass of water in the coffee cup calorimeter was measured and recorded some of the water evaporated. The lid was not placed on the coffee cup calorimeter during the experiment. The mass of the metal was measured incorrectly. The actual mass of the metal used was greater than what was recorded. The "final" temperature was read before the metal and water had reached equilibrium The calorimeter used in…
A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q = specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 °C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the sblution increases to 30.0 °C At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, qp; that is, Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water (4.18 J/(g. °C)J, that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. ΔΗp Express the…
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
A east.cengagenow.com/ilrn/takeAssignment/takeCXPCompliantActivity.do?locator=Dassignment-take References Use the References to access Important values If needed for this question. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.5021 g sample of heptadecanoic acid (C,,H,0,) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.246x10 g of water. During the combustion the temperature increases from 21.91 to 25.07 °C. The heat capacity of water is 4.184 Jg1°C1. tin The heat capacity of the calorimeter was determined in a previous experiment to be 822.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. Cmbe te car C,,H3402(s) + (49/2) O2(g) → 17 H2O(1) + 17 CO2(g) + Energy kJ/mol Molar Heat of Combustion = Save and Exit Cengage Learning | Cengage…
2. a. Determine the standard heat of formation, AH for the following reaction using the Data from the Table. C3H12 ) + 802(g) → 5CO2 + 6H₂O b. State whether the reaction is exothermic or endothermic. Explain. c. Rewrite the equation as thermochemical equations in two different ways to include the heat calculated in (2a). d. Draw a detail Energy Diagram representing the thermochemical equation in Ⓒ illustrating the the reactants and products and their positions.