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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The rise in atmospheric carbon dioxide results in higher concentrations of dissolved carbon dioxide in natural waters. Use Henry's law and the data as given to calculate the solubility of CO2 in water at 25 °c when its partial pressure is (a) 3.8 kPa. (b) 50.0 kPa.
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.
The feed gas to a methanol synthesis reactor consists of %75 mol H2, %12 mol CO, %8 mol CO2 and %5 mol N2. The system comes to equilibrium at 550 K and 100 bar according to the reactions given in the appendix. Calculate the equilibrium composition of the mixture, assuming the ideal gas and the temperature-independent reaction enthalpy.
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?
(ii) Explain the reasoning for using compromise temperature and pressure in industrial processes
Kindly assist with question 5(a)(i)(ii)(iii) Thanks in advance
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 =
The reactionSO2(g) + 2 H2S(g) ⇌ 3 S(s) + 2 H2O(g)is the basis of a suggested method for removal of SO2 frompower-plant stack gases. (a) What is the equilibriumconstant for the reaction at 298 K? (b) In principle,is this reaction a feasible method of removing SO2?(c) If PSO2 = PH2S and the vapor pressure of water is 25 torr,calculate the equilibrium SO2 pressure in the system at298 K. (d) Would you expect the process to be more orless effective at higher temperatures?
(b) A motor car tyre contained a fixed mass of air at 27 °C. Its pressure was 220 k Nm-4 abe atmospheric pressure. After a 60-minute drive, the air pressure rose to 250 k Nm-2 above atmospheric pressure. What was the new temperature of the air in the tyre, in degrees Celsius, if the volume of air remained constant? Note: (Atmospheric pressure = 100 k N m-2)
Im confused how do i solve?
6) Calculate the final temperature of a sample of carbon dioxide of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm³ at 298.15 K to 2.00 dm³.

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