(a)
Interpretation:
Calculate the required heat input.
Concept introduction:
The open-system energy balance equation is,
Where,
(b)
Interpretation:
Calculate the required heat input and explain the physical significance of the calculated values.
Concept introduction:
The open-system energy balance equation is,
Where,
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Chapter 7 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- = 1. A process has been proposed whereby an ideal gas is taken from P 10 bar and T = 300 K to P = 1 bar and T = 500 K in a closed system. During the process the system (ideal gas) does 1,000 kJ of work and receives 5,430 kJ of heat from the surroundings. The temperature of the surroundings is constant at 300 K. Ideal gas heat capacity: (b) Cp R = 3.6 +0.5 10-³T (T in K) Calculate the change in entropy of the gas.arrow_forward4. The heat capacity of solid lead oxide is given by the equation: Cp(T) = 44.35 + 1.47 × 10-3 xT with T in units of K and the resulting Cp(T) in units of K-mol Calculate the change in enthalpy of 1 mole of PbO(s) if it is heated from 200 to 600 K at constant pressure. (Assume no phase transitions take place during this process.)arrow_forwardOne mol of an ideal gas is heated at a constant external pressure of 200 kPa. Calculate the enthalpy involved and change in internal energy during this process upon the temperature change from 100 oC to 25.0 oC. Molar specific heat capacity CV = 3/2 R and the universal gas constant is 8.3145 J‧mol-1·K-1.arrow_forward
- Suppose a piece of solid lead weighing 41.3 g at a temperature of 312 °C is placed in 413 g of liquid lead at a temperature of 374 °C. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is AH fus = 4.77 kj mol¹ at its melting point of 328 °C, and the molar heat capacities cp of solid and liquid lead are 26.9 and 28.6 J K¹ mol-¹, respectively. (Enter your answer to three significant figures.) T₁= Jc Submit Answer Try Another Version 1 item attempt remainingarrow_forwardCalculate the heat (q) and the work (w) in Joules, which the system exchanges with the return process in which the pressure is constant at 100 kPa. The initial temperature is 300 K and a final 500 K. The system contains 2 g of gas, which behaves in the state field the equation of an ideal gas and its molar heat capacity is cp, m = 43.0 J/g K. cv = 0.0346 J/g. Karrow_forwardA 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 %3D specific 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 constant R.°arrow_forward
- P2.30 A 1.75 mol sample of an ideal gas for which Cv.m = 3R/2 undergoes the following two-step process: (1) From an initial state of the gas described by T = 15.0°C and P = 5.00 X 104 Pa, the gas undergoes an isothermal ex- pansion against a constant external pressure of 2.50 × 104 Pa until the volume has doubled. (2) Subsequently, the gas is cooled at constant volume. The temperature falls to -19.0°C. Calculate q, w, AU, and AH for each step and for the overall process.arrow_forwardThree cubic meters of a 1.5 molar aqueous sulfuric acid solution (SG=1.064) is stored at 25∘C. Determine the standard heat of formation of the solution in kJ/mol H2SO4 relative to the solute elements and water, as well as the total enthalpy of the solution relative to the same reference conditions.arrow_forwardCalculate the value of cp at 298 K and 1 atm pressure predicted for Cl, and NO, by the classical equipartition theorem. (Enter your answers to at least two decimal places.) Cp(Cl)) = J mol 1 K1 Cp(NO,) = J mol K1 The actual heat capacities of C and NO, are 33.91 and 36.97 J molK, respectively. Calculate the fraction (expressed as a percentage) of the measured value that arises from vibrational motions. vibrational contribution to cp(Cl,) = vibrational contribution to cp(NO,) =arrow_forward
- The integrated form of Kirchhoff's Law: A, H(T2) = A,H(T;) + A,Cp(T2 - T) where A,H(T;) and 4,H(T2) are the reaction enthalpies at temperatures T; and T2 respectively and A,Cp is the heat capacity of the reaction works based on the assumption that: A. For extremely large temperature changes, the heat capacity of the reaction can be assumed independent of temperature. B. For extremely large temperature changes, the heat capacity of the reaction increases linearly as a function of temperature C. For extremely small temperature changes, the heat capacity of the reaction can be assumed independent of temperature D. For extremely small temperature changes, the heat capacity of the reaction increases linearly as a function of temperature O E. Both (B) and (C)arrow_forward1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.arrow_forwardFrom the data in Table 2C.4 of the Resource section, calculate ΔrH⦵ and ΔrU⦵ at (i) 298 K, (ii) 478 K for the reaction C(graphite) + H2O(g) → CO(g) + H2(g). Assume all heat capacities to be constant over the temperature range of interest.arrow_forward
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