5. Calculate the work done by a piston with diameter d =0.1m which moves from x, =0.15 m to x, = 0.3m (see the next figure). The gas is under initial pressure po =12MPA. The process of gas expansion is isothermal, which means that at any moment during the expansion, pV =C holds, where p is the current pressure of the gas, V is the current volume and C is a constant. P.=12MPA d=0.1

5. Calculate the work done by a piston with diameter d =0.1m which moves from x, =0.15 m to x, = 0.3m (see the next figure). The gas is under initial pressure po =12MPA. The process of gas expansion is isothermal, which means that at any moment during the expansion, pV =C holds, where p is the current pressure of the gas, V is the current volume and C is a constant. P.=12MPA d=0.1

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...

See similar textbooks

Similar questions

(2) The following diagram represents the P – V changes of a gas. Write an expression for the total work done. V2 V3 V
Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2 NaN, (s) 2 Na(s) + 3 N₂(g) Calculate the value of work, w, for the system if 18.5 g NaN, reacts completely at 1.00 atm and 22 °C. W = -10471.0771 Incorrect V JE JO B MacBook Air H N M ( 9 19 ) J
(1 L atm = 101.325 J, 1 L bar = 100.000 J) ii) A gaseous mixture was enclosed in a piston and cylinder system having a volume of 8.545 L. When a chemical reaction occurred, the volume increased to 4.375 L and 0.563 calories of heat was released. The external pressure was 0.9986 bar. Calculate the change in enthalpy, work, and the change in internal energy for this system in kJ.
Consider the reaction 2 N20 (g) – 2N, (g) + 02 (g). Calculate the work in kJ units at T= 320.0 K (in kJ and in 4 Significant Figures with a positive or negative sign). (Gas constant = 8.3145 J/mol K). No need to write kJ. Answer would be something like +3440 or -3442 or +23.21 or -23.21
F 8. A 3.50 mole sample of an ideal gas with Cv= 3R/2 undergoes reversible expansion. The initial temperature and pressure are T1 = 310 K and P1 = 15.2 bar. The final pressure is P2 = 1.45 bar. Calculate ΔU in kJ for this process. (First calculate T2) Please show all steps.
For the reaction 2N₂(g) + O2(g) → 2N₂O(g) AG = 214 kJ and AS = -148.5 J/K at 334 K and 1 atm. This reaction is product favored under standard conditions at 334 K. The standard enthalpy change for the reaction of 1.51 moles of N₂ (9) at this temperature would be For the reaction 2H₂O(1)→ 2H₂(g) + O₂(g) AG=483 kJ and AH = 572 kJ at 273 K and 1 atm. This reaction is reactant favored under standard conditions at 273 K. The entropy change for the reaction of 2.18 moles of H₂O(1) at this temperature would be kl. J/K.
6600 J of heat flow into 0.014 m³ of a monatomic gas at 1.5 x 105 N/m?. The gas expands isothermally to 0.058 m. How much work is done on the gas in Joules? Energy entering the gas as work is +, Energy leaving as work is-. Work = J %3D
Calculate the work done (J) by 2 mole of an Oplg) when it expands reversibly at a constant pressure of 4 atm. The temperature of the gas is found to increase from 268 to 300 K.
What is the value of the work for a system if the work done by the system is it expanding from 8.50 L to 91.6 L against a pressure of 0.992 atm? Select one: a. 8.35 kJ b. 83.1 kJ C. -82.4 kJ d. -83.1 kJ е. -8.35 kJ f. -8.24 x 10^4 kJ g. 82.4 kJ h. none of these i. 8.35 x 10^3 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?
4
As a 1.00-mol sample of a monatomic ideal gas expands adiabatically, the work done on it is -2.50 × 103 J. The initial temperature and pressure of the gas are 500 K and 3.60 atm. Calculate (a) the final temperature and (b) thefinal pressure.