Please answer question 9 part A Calorimetry is a method used to measure changesin enthalpy, or heat, that occur during chemicalprocesses. Two common calorimeters are constant-pressure calorimeters and constant-volume (or"bomb") calorimeters. Bomb calorimeters are usedto measure combustion and other gas-producingreactions, in which the reaction is observed in astrong, sealed vessel. A simple constant-pressurecalorimeter can be made from a foam coffee cupand a thermometer, in which energy changes in areaction are observed via the change intemperature of the solution in the cup. The ideabehind calorimeters is that if they are sufficientlyinsulated from the outside environment, any energyPart AIn the following experiment, a coffee-cup calorimeter containing 100 mL of H20 is used. The initial temperature of thecalorimeter is 23.0 °C. If 5.70 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solutionin the calorimeter? The heat of solution AHsoln of CaCl2 is –82.8 kJ/mol.Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: Cs = 4.184J/g.°C.Express your answer with the appropriate units.he chemical reaction will begained or lostdirectly observable as a temperature and/orpressure change in the calorimeter.• View Available Hint(s)HẢ?ValueUnits

100ml of H2O is used Initial Temperature = 23oC ∆H = -82.8kJ/mol = 82800J Specific heat = 4.184J/goC…

In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 °C. If 5.70 g of CaČl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution AHsoln of CaCl2 is –82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184 J/g.°C. Express your answer with the appropriate units. • View Available Hint(s) ? Value Units

In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 °C. If 5.70 g of CaČl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution AHsoln of CaCl2 is –82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184 J/g.°C. Express your answer with the appropriate units. • View Available Hint(s) ? Value Units

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 18P

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Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
In a constant-pressure calorimeter that is, one that expands or contracts if the volume of the system changes, 0.145 mole of an ideal gas contracts slowly from 5.00 L to 3.92 L. If the initial temperature of the gas is 0.0 C, calculate the U and w for the process.
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) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.
o-phthalic acid, C8H6O4, is sometimes used as a calorimetric standard. Its heat ofcombustion is - 3.224 × 103 kJ/mol C8H6O4. From the following data determine theheat capacity of a bomb calorimeter assembly (i.e., of the bomb, water, stirrer,thermometer, wires, etc.)mass of o-phthalic acid burned: 1.078 ginitial calorimeter temperature 24.96 °Cfinal calorimeter temperature 30.76 °C
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
What does q with subscript p mean in relation to Constant pressure calorimetry? it seems to mean that if you're in a constant pressure environment, that the calculation of how he flowed, q, is equal to the change in enthalpy. From my reading it also seems to mean that this is only the case and a constant pressure enviriment. if P constant than in a rxn, q = s m change temp = enthalpy of reaction, another term for "heat flow of reaction".
A sample of solid biphenyl weighing 0.5260 g was ignited in a bomb calorimeter initially at 25.0°C, producing a temperature rise of 1.910 K. Determine the internal energy (∆U) of combustion. To properly determine the internal energy of combustion for the solid biphenyl, the calorimeter was first calibrated. a)A 0.7750 g sample of benzoic acid (C₆H₅COOH, MW 122.1 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.940 K. For benzoic acid, the internal energy combustion at constant volume, ∆U, is known to be –3226 kJ/mol. Calculate the calorimeter constant, in kJ/K. b)using the caloremeter constant, determine triangleU, in KJ/mol, for the conbustion of solid biphenyl ((C6H5)2, MW 154.21 g/mol)
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)?