A gas in the initial state of p1 = 75 psia and V1 = 5 ft.3 undergoes a process to p2 = 25 psia and V2 = 9.68 ft., during which the enthalpy decreases 62 BTU. The%3Dspecific heat at constant volume is c, = 0.754 BTU/lb.°R. Determine (a) the change of internal energy, (b) the specific heat at constant pressure, (c) the gas constantR.°

Here we have provided change in enthalpy and we have to calculate the internal energy change. We…

Answered: A gas in the initial state of p1 = 75…

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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4b. Combustion of 3.500 g of butane gas (C4H10; Mm = 58.12 g/mol) causes a temperature rise (AT) of 29.09°C in a constant-pressure calorimeter that has a heat capacity (C,) of 5.500 kJ/°C. o Use calorimetry to calculate the heat (q,) released by the combustion of 3.500 g of butane gas in the calorimeter Яр [ Select ] kJ / 3.500 g of C4H10 o Use the heat (qp) released by the combustion of 3.500 g of butane gas, calculated in part (a) to calculate the change in enthalpy (AHrxn) for the following reaction. (for 1 mole of butane gas): C4H10(9) + 13/2 02(9) → 4 CO2(9) + 5 H20(g) AHrxn [ Select ] kJ / mol of C4H10 • Use the heats of formation (AH¢°) to calculate the change in enthalpy (AHrxn) for the same reaction. (for 1 mole of butane gas): Heats of Formation: CO2 (g) - A H°f = -393.5 kJ/mol H2O(g) - A H°f = -241.8 kJ/mol O2 (9) - A H°f 0.0 kJ/mol C4H10 (g) - A H°f = -125.6 kJ/mol C4H10(g) + 13/2 02(g) → 4 CO2(9) + 5 H20(g) ΔΗη [ Select ] kJ / mol of C4H10
The thermite reaction, used for welding iron, is the reaction of FegO4 with Al. 8 Al (s) + 3 Fe3O4 (s) > 4 Al203 (s) + 9 Fe (s) AH° = -3350 kJ Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000°C. How much heat (in kJ) is released by the reaction of 16.5 g of Al with 76.7 g of Fe304? Enter your numerical answer in units of kJ.
(2B) A heat engine operates between a hot source at 130.°C and a cold sink at 10.°C. How much workcan be done by the engine if 523 kJ of heat are extracted from the hot source?
None
The combustion of 0.150g of ethanol, CHOH(1) 2 5 releases 4.47kJ of heat. The molar enthalpy of combustion of liquid is?
The internal pressure of a gas, π = au dv)T' is a measure of intermolecular forces, because it indicates a change in internal energy as the molecules get closer or further apart, without temperature changing. = a Calculate the change in internal 1 Vm T energy, AU, when 1.5 mols of acetone (a = 16 l² atm/mo1²), expands from 2 liters to 5 liters at a constant temperature. ii) Would this change in internal energy be greater or smaller for an ideal gas? Why? i) Using the van der Waals equation of state, T = au
81.6 g of a metal alloy was heated to 93 o C, then plunged into 105 mL of H 2O that was at 19.5 o C. The system equilibrated at 22.3 oC. What is the specific heat of the metal?
The standard heat of formation, AH;, is defined as the enthalpy change for the formation of one mole of Part B substance from its constituent elements in their standard states. Thus, elements in their standard states have AH: = 0. Heat of formation values can be used The combustion of ethene, C2H4, occurs via the reaction to calculate the enthalpy change of any reaction. C2H4 (g) + 302 (g)→2CO2(g) + 2H20(g) Consider, for example, the reaction with heat of formation values given by the following table: 2NΟ (5) + Ο, (s) 2ΝO, (g) ΔΗρ (kJ/mol) Substance with heat of formation values given by the following table: C2H4 (g) 52.47 CO2 (g) -393.5 Substance (kJ/mol) H2O(g) -241.8 NO(g) 90.2 Calculate the enthalpy for the combustion of ethene. 02 (g) Express your answer to four significant figures and include the appropriate units. NO2(g) 33.2 • View Available Hint(s) Then the heat of formation for the overall reaction is ΔΗ ΔΗ (products) -ΔΗ; (reactants ) [2(90.2) + 0] HA ? 2(33.2) -114 kJ/mol…
3. The enthalpy change of a reaction Hrxn equals heat q, if the reaction is performed ... (A) in a closed system (B) in an isolated system (C) at constant volume (D) at constant temperature (E) at constant pressure

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