for the reactionCr(C6H6)2 (s) → Cr(s) + 2 C6H6 (g)ArU© (583K) = + 8.0 kJmol-1.find the corresponding reaction enthalpy andestimate the standard enthalpy of formation ofCr(C6H6)2(is) at 583K. The constant-pressuremolar heat capacity of benzene is 81.67 JK-1 mol-1 as a gas. The heat capacities of graphite andhydrogen are approximately constant in thistemperature range.

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Answered: for the reaction Cr(C6H6)2 (s) → Cr(s)…

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 67AP

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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.
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 Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.
Estimate the standard internal energy of formation of liquid methyl ethanoate, CH3COOCH3, at 298 K from its standard enthalpy of formation, which is -442 kJ mol-1.
A sample of the sugar d-ribose (C5H10O5) of mass 0.727 g was placed in a calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K. In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid, for which the internal energy of combustion is −3251 kJ mol−1, gave a temperature rise of 1.940 K. Calculate the enthalpy of formation of d-ribose.
Use the molar constant volume heat capacities for gases given in Topic 4C (as multiples for R) to estimate the change in reaction enthalpy of N2 (g) + 3 H2 (g) ---> 2 NH3 (g) when the temperture is increased from 300. K to 500. K. Ignore the vibrational contributions to heat capacity. Is the reaction more or less exothermic at the higher temperature? Atoms Linear Molecules Nonlinear Molecules Cv,m 3/2 R 5/2 R 3 R Cp,m 5/2 R 7/2 R 4 R
3. What is the change in entropy associated with heating water from 15 ºC to 55 ºC? The constant volume heat capacity of water is CV,m = 75.3 J/mol K, and is constant over this temperature range.
To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO andHCl.2. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol, calculate the %error.
The temperature of a block of iron (Cv,m = 25.1 J K-1 mol- 1) of mass 1.4 kg fell by 65 °c as it cooled to room temperature.What is its change in internal energy?
Use values of standard enthalpies of formation, standard entropies, and standard heat capacities available from tables in the Resource section to calculate the standard enthalpy and entropy changes at 298 K and 398 K for the reaction CO2(g) + H2(g) → CO(g) + H2O(g). Assume that the heat capacities are constant over the temperature range involved.
A) For nitrogen gas the values of Cv and Cp at 25°C are 20.8 J K−1 mol−1 and 29.1 J K−1 mol−1, respectively. When a sample of nitrogen is heated at constant pressure, what fraction of the energy is used to increase the internal energy of the gas? B) How much energy (in KJ) is required to raise the temperature of 136.4 g N2 from 25.0°C to 87.0°C in a vessel having a constant volume?
It is often useful to be able to anticipate, without doing a detailed calculation, whether an increase in temperature will result in a raising or a lowering of a reaction enthalpy. The constant-p ressure molar heat capacity of a gas of linear molecules is approximately (7)/(2) R whereas that of a gas of nonlinear molecules is approximately 4R. Decide whether the standard enthalpies of the following reactions will increase or decrease with increasing temperature:(a) 2 H2(g) + O2(g) → 2 H2O(g)(b) CH4(g) + 2 O2(g) → CO2( g) + 2 H2O(g)(c) N2(g) + 3 H2(g) → 2 NH3(g)

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