2 C,H,0(g) + 50,(8)4 CO2(g) + 4 H,0(g)Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values youcalculate may not exactly match published values for this reaction.exothermicIs this reaction exothermic, endothermic, or neither?endothermicO neitherIf you said the reaction was exothermic or endothermic, calculate the amount of heat that wasreleased or absorbed by the reaction in the second experiment.kJkJCalculate the reaction enthalpy AH,per mole of C,H¸0.rxnmol A student runs two experiments with a constant-volume "bomb" calorimetercontaining 1300. g of water (see sketch at right).thermometerstirrerFirst, a 5.500 g tablet of benzoic acid (CH,CO,H) is put into the "bomb" andwaterburned completely in an excess of oxygen. (Benzoic acid is known to have a heat ofcombustion of 26.454 kJ/g.) The temperature of the water is observed to rise frominsulation23.00 °C to 47.33 °C over a time of 5.8 minutes.Next, 4.150 g of acetaldehyde (C,H,0) are put into the "bomb" and similarlycompletely burned in an excess of oxygen. This time the temperature of the waterrises from 23.00 °C to 42.14 °C.chemical reaction"bomb"A "bomb" calorimeter.Use this information, and any other information you need from the ALEKS Dataresource, to answer the questions below about this reaction:2 C,H,0(g) + 50,(g) →4 CO2(g) + 4 H20(g)Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values youcalculate may not exactly match published values for this reaction.

a) Now, after the combustion of acetaldehyde in bomb calorimeter, the temperature of water rises…

exothermic Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. | kJ kJ Calculate the reaction enthalpy AH, rxn per mole of C,H,0. mol

exothermic Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. | kJ kJ Calculate the reaction enthalpy AH, rxn per mole of C,H,0. mol

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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2. Calculate the amount of heat required to raise the temperature of 950.0 mL of a solution from 22.5 °C to 38.0 °C if the solution has a density of 1.04 g mL-l and a heat capacity of 4.08 J K-l g. 3. This reaction: CH4(g) + 202(g) → CO2(g) + 2H2O(1) produces 56.0 kJ of heat when 1.00 g of methane is burned. What is the molar heat of combustion for CH4? 4. In thermodynamics heat is represented by the letter 'q' and q is negative for processes which lose heat to the surroundings (i.e. exothermic processes). What is q for burning one mole of methane? 5. What mass of methane would need to be burned in order to generate the heat required to raise the temperature of the solution in question 2? (Hint: look at question 3 for some relevant data) 6. In this lab class you will measure the enthalpy change for hydrochloric acid reacting with sodium hydroxide. What effect, if any, would using nitric acid instead of hydrochloric acid have on the enthalpy changes measured in this experiment? Why?…
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 323. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -162. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? kJ exothermic O endothermic x10 X 3
4. In a coffee-cup calorimeter, 3.20 g of NH4NO3 is mixed with 86.00 g of water at an initial temperature of 23.53°C. After dissolution of the salt, the final temperature of the calorimeter contents is 21.32°C. Assuming the solution has a heat capacity of 4.184 J/g °C and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
In a coffee cup calorimeter, 40.0 mL of 0.33 M nitric acid (HNO3) and 40.0 mL of 0.33 M potassium hydroxide (KOH) are mixed to observe the heat released during the neutralization reaction. Based on the data in the table, what is the enthalpy of the neutralization reaction between HNO3 and KOH? Initial temperature in the calorimeter (°C) Final temperature in the calorimeter (°C) Final mass of the neutralized solution (g) Calorimeter constant (J/C)) 21.3 23.5 79.74 4.57
In a constant-pressure calorimeter, 55.0 mL of 0.350 M Ba(OH), was added to 55.0 mL of 0.700 M HCI. The reaction caused the temperature of the solution to rise from 23.81 °C to 28.58 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. AH= kJ/mol H₂O
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?
The reaction below is a exothermic or endothermic reaction. 2SO3(g) + Heat ⇋ 2SO2(g) + O2(g)
113 kJ of heat is absorbed when one mole of carbon reacts with one mole of water. Energy + C + H2O → CO + H2 According to the reaction above it can be concluded that the reaction is a endothermic, because the change of enthalpy was negative b exothermic, because the change of enthalpy was negative c exothermic, because the change of enthalpy was positive d endothermic, because the change of enthalpy was positive
The heat of reaction for the reaction A + 2B → 2C is 1200. kJ.The heat of reaction for the reaction B + D → C is 150. kJ.Using Hess's Law, calculate the heat of reaction for the reaction A → 2D.
Determine the mass of water that is produced when 673 kJ of heat is absorbed in the following reaction? H₂A (s) + 2 XOH (ag) --> X₂A (aq) + 2 H₂O (g) AH = 448.4 kJ You may or may not need the following molar mass information: H₂O molar mass = 18.01 g/mol X₂A molar mass = 113.24 g/mol Report with the correct number of significant figures. Include the correct unit. Your Answer: Answer units
True or False: The test tube in which a chemical reaction is taking place feels warmer to the touch. The reaction is endothermic.