A 1 - kilogram mass is attached to a spring whoseconstant is 1 N/m, and the entire system is thensubmerged in a liquid that imparts a damping forcenumerically equal to the instantaneous velocity.Determine the equations of motion. (a) the mass isinitially released from rest from a point 1 meter belowthe equilibrium position x(t)=has a downward velocity of 5 m/s x(t)_m (b) the mass=m

Step 1: Concept and general expression Step 2: part (a) Step 3: part (b)

Answered: A 1 - kilogram mass is attached to a…

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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In the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and is
In the gas phase reaction 2 A(g) + B(g) = 3 C (g) + 2 D (g) it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate (a) the mole fractions of each species, (b) KX, (c) KP and (d) △Go . Answer: [0.087 (A); 0.370 (B); 0.196 (C); 0.348 (D); 0.326; 0.325; 2.76 kJ]
The equilibrium constant for the reaction N2(g) + O2(g) -2 NO(g) is 1.7 x 101 at an elevated temperature. A reaction vessel at this temperature contains N2(g) at a partial pressure of 0.25 bar, O2(g) at a partial pressure of 0.25 bar, and NO(g) at a partial pressure of 4.2 x 10- bar. Select the one true statemnent for this system. The reaction quotient Q is smaller than K, and the reaction proceeds to the reactants side. O The reaction quotient Q is larger than Kand the reaction proceeds to the reactants side. O The reaction quotient Q is smaller than K, and the reaction proceeds to the products side. The reaction quotient Q is larger than K, and the reaction proceeds to the products side. The system is at equilibrium.
A study of air quality in a particular city by an environmental group suggests that t years from now, the level of carbon monoxide, in parts per million, in the air can be modeled by the function A(t) : 0.2t2 + 0.1t + 5.1.
For the two following cases, calculate the composition and partial pressures of a system in which nitrogen and hydrogen are mixed at initial partial pressures of 1.00 bar and 4.00 bar and allowed to reach equilibrium with their product ammonia at 400 K. (a) Assume that the total pressure is constant. (b) Assume that the total volume is constant. [The equilibrium constant is K=5.97 at 400 K.]
A mixture of 0.02993 mol of Og, 0.02165 mal of NOCI, 0.02691 mol of NOz, and 0.01037 mol of Cly is placed in a 1.0-L steel pressure vessel at 2385 K. The following equilibrium is established: 1 0,(9) + 2 NOC(g) =2 NO;(9) + 1 Ciy(9) At equilibrium 0.008268 mol of Clz is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Oz, NOCI, NOz, and C. Peg(0) - Peg(NOCI) = Pa(NO,) Pa(C) - (b) Calculate Ke for this reaction.
For this heterogeneous system 2A(aq)+3B(g)+C(l)↽−−⇀2D(s)+3E(g) the concentrations and pressures at equilibrium are [A]=1.35×10−2 M, ?B=8.62×103 Pa, [C]=14.93 M, [D]=12.55 M, and ?E=5.86×104 torr. Calculate the thermodynamic equilibrium constant, ?. please type in words don't image upload thank you.
(a)At 0 oC, liquid water and ice are in equilibrium at standard pressure, so they have the SAME molar Gibbs energy. When raise from 1.0 bar to 100 bar, how much Gibbs free energy change in the liquid phase ? (molar mass of water 18 g mol-1; mass density of ice = 0.9150 g cm-3; mass density of liquid water, 0.9999 g cm-3) Set the initial Gibbs energy = 0 if you like. (b) how much Gibbs free energy change in the solid phase? c) under this process according to your calculation , solid changes to liquid. Liquid changes to solid
(ii) Explain the reasoning for using compromise temperature and pressure in industrial processes
Calculate (a) the (molar) Gibbs energy of mixing, (b) the(molar) entropy of mixing when the two major componentsof air (nitrogen and oxygen) are mixed to form air at 298 K.The mole fractions of N2 and 0 2 are 0.78 and 0.22. respectively. (c) Is the mixing spontaneous?
Suppose now that argon is added to the mixture in the previous exercise to bring the composition closer to real air, with mole fractions 0.780. 0.210, and 0.0096, respectively. (a) What is the additional change in molar Gibbs energy and entropy at 298 K? (b) Is the mixing spontaneous?
5) Starting from the expression Cp – G, = T (P/ər), (V/ar). ' use the appropriate relations between partial derivatives to show that T(V/ar), Cp – Cy =

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