Solution calorimetry was used to study the acid-catalyzed addition of water to 1- butene: CH3-CH2-CH=CH2 + H2O-> CH3-CH2-CH2-CH2-OH When 5.000 g of butene reacted with excess water the temperature change was 0.250 °C. The electrical calibration run after the reaction gave the following values: En = 12.00 V, E, 1.200 V, t = 60.0 s, AT = 0.15°C. %3D !3! Calculate the molar enthalpy change for the reaction.

Solution calorimetry was used to study the acid-catalyzed addition of water to 1- butene: CH3-CH2-CH=CH2 + H2O-> CH3-CH2-CH2-CH2-OH When 5.000 g of butene reacted with excess water the temperature change was 0.250 °C. The electrical calibration run after the reaction gave the following values: En = 12.00 V, E, 1.200 V, t = 60.0 s, AT = 0.15°C. %3D !3! Calculate the molar enthalpy change for the reaction.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.83E: Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant...

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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.
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:
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 released/absorbed by the reaction (qrxn) between nitric acid and potassium hydroxide. Express your answer in kJ. Given: A newly made Styrofoam ball calorimeter was first calibrated by mixing in it 10.0 mL of 0.40 M hydrochloric acid and 0.1008 g magnesium oxide (MW = 40.30 g/mol; specific heat = 0.276 kJ/g°C). The reaction enthalpy (ΔHrxn) of HCl and MgO is -139.6 kJ/mol. The temperature change was recorded to be 5.5 °C. After calibration, the calorimeter was used to determine reaction enthalpy of nitric acid and potassium hydroxide by mixing in it 5.0 mL of 0.40 M HNO3 and 5.0 mL of 0.80 M KOH. The temperature change was recorded to be 1.0 °C.
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)?
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: HCl (aq) + NaOH(aq) à NaCl(aq) + H2O(l)
The formulas give the enthalpy when Coal and Methane react with oxygen:C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJCH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4gives 44 gram of CO2+891kJ 1-Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg.Calculate the lower heating value for Methane. 2-Calculate the amount of CO2 which is produced per kWh for Coal and Methane
For the following combustion reaction of benzoic acid (HC7H5O2; molar mass = 122.1 g/mol) HC7H5O2(s) + 15/2 O2(g) --> 7CO2(g) + 3H2O(l); DHcomb = -3226 kJ 1.00 g of benzoic acid is combusted in a bomb calorimeter, which contains 1.00 kg of water (specific heat = 4.184 J/g.oC) and the bomb has a heat capacity of 890 J/oC. If the initial temperature of the calorimeter is 25.0oC, what is the final temperature of the calorimeter when the combustion is completed? (A) 51.8oC (B) 31.3oC (C) 30.2oC (D) 27.0oC
1. Calculate the standard enthalpy of formation of C10H10. Its standard enthalpy of combustion is shown by the equation: 2C10H10 (l) + 25O2 (g) → 20CO2 (g) + 10H2O (l) ∆H = 10,314 KJ/mol The standard heat of formation (KJ/mol) at 298.15oC : CO2 = -393.5 ; H2O(l) = -285.8 2. Determine ΔG° at 298.15K for the reaction: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Given that ΔH° = -1648 kJ ; ΔS° = -549.3 J/K 3. In the picture, Find the the ∆H°rxn if ∆G°rxn is 420 kJ/mol and ∆S°rxn is -143 J/mol*k
The difference between heats of reaction at constant pressure and constant volume for the reaction:2C6H6(l) + 15O2(g) = 12CO2(g) + 6H2O(l) at 298K in kJ isA. -7.43 kJB. 3.72 kJC. -3.72 kJD. 7.43 kJ
Nitroglycerin (C3H5N3O9), a liquid at room temperature (25 oC) and atmospheric pressure (1.01325 x 105 Pa) is used to relieve angina. It may undergo decomposition under these same conditions to form nitrogen, carbon dioxide, oxygen and water, with an enthalpy of decomposition of -1541 kJ mol-1.The standard enthalpies of formation of water and carbon dioxide are -285.9 kJ mol-1 and -393.5 kJ mol-1 respectively. Determine the standard enthalpy of formation of 1.0 mole of nitroglycerin.
The following formulas give the enthalpy, when Coal and Methane react with oxygen: C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJ CH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4 gives 44 gram of CO2+891kJ a) Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg. b) Calculate the amount of CO2 which is produced per kWh for Coal and Methane. Give it in kg/kWh.