Using the bond energies in the table below, estimate the enthalpy change in kJ/mol corresponding to the following reaction for the addition of X2 across the C-C double bond in ethene. X could be F, CI, Br, or I; the drawings are for the example of X being I (iodine). + I-I Ethene lodine Diiodoethane Bond strength (kJ mol-1) 613 339 405 363 239 Bond C=C C-C C-H C-X X-X Show your work using the abc format by uploading supporting information to Final Exam Workings. Your Answer: Answer units

Using the bond energies in the table below, estimate the enthalpy change in kJ/mol corresponding to the following reaction for the addition of X2 across the C-C double bond in ethene. X could be F, CI, Br, or I; the drawings are for the example of X being I (iodine). + I-I Ethene lodine Diiodoethane Bond strength (kJ mol-1) 613 339 405 363 239 Bond C=C C-C C-H C-X X-X Show your work using the abc format by uploading supporting information to Final Exam Workings. Your Answer: Answer units

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

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When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…
When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…
An English chemistry professor needs a cup of hot tea before grading 50 homeworkassignments but his electric water heater is broken . In his lab, however, he doeshave some ethanol (CH3CH2OH, MW=46.07gmol-1) and 1 gram of benzoic acid(C6H5COOH, MW=122.12 gmol-1). He knows that the benzoic acid has an enthalpyof combustion, H, of -3226.7 kJmol-1. In a constant volume (bomb) calorimeterinitially at 293.15 K, he finds that the combustion of 1.000 g of benzoic acidincreased the temperature to 297.67 K. In the exact same calorimeter, 1.000 g ofethanol raised the temperature from 293.15K to 298.38K.(a) What is the enthalpy of combustion for 1 mole of ethanol? I am confused about this question and I need help.
A quantity of 1.00 x 102 mL of 0.500 M HCl was mixed with 1.00 x 102 mL of 0.500 M NaOHin a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCLand NaOH solutions was same, 22.50 0C, and the final temperature of the mixed solution was25.86 0C. Calculate the (a) heat of the reaction at constant pressure (qp) and (b) the change inenthalpy for the neutralization reaction (ΔHrxn) in kJ per mole of HCl. Assume that the densitiesand specific heat of the solutions are the same as for water (1.00 g/mL and4.184 J/g.0C, respectively).NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
Calculate the ΔH°f of C6H12O6(s) from the following data: Show the complete and step by step solution ΔH combustion of C6H12O6(s) = -2816kJ/mol ΔH°f of CO2 (g) = -393.5 kJ/mol ΔH°f of H2O (l) = -285.9 kJ/mol Equation: C6H12O6(s) + O2(g) -> CO2(g) + H2O(l)
The specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?
A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0125 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.4ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.
At constant pressure and 25^C, What is delta H for the following reaction. 2C2H6(g) + 7O2(g) = 4CO2(g) + H2O(l) if the complete consumption of 38.2 g of C2H6 libraties 1981 KJ of heat energy?
According to Schwabe and Wagner, the heats of combustion in a constant-volume calorimeter for fumaric and maleic acids are -1337.21 kJ mol-1 and -1360.43 kJ mol-1, respectively, at approximately 25 °C. What is the enthalpy of isomerization of maleic acid into fumaric acid in kJ mol-1?
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm3 of 1.0 moldm-3 of Nitric Acid (HNO3) and 50.00 cm3 of 1.0 moldm-3 of Potassium Hydroxide (KOH) are mixed? According to your simulation, the temperature rose by __6.81__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1)
Calculate the heat of reaction of each reaction: (assume density of solution is 1.04 g/ml and specific heat of solution is = 3.89 Jg-1K-1) qreaction = -[(∆T x m x cp) + (Cp x ∆T)] I calculated Cp as 429.04 DeltaT: 4 deg C Products: 50 mL of 1.0 M HCl and 50 mL of 1.0 M of NaOH