What is the equilibrium number of vacancies, per cubic metre, for copper at 628 °C.Given:Activation energy per vacancy = 0.8 eV/atomAtomic weight of copper = 58.5 g/mol and density at the given temperature is 8.40 g/cm³Boltzmann's constant kg= 1.38×10-23 J/atom.K = 8.62x10-5 eV/atom.KYour answer should be in scientific notation with 5 significant figures. The following example shows the format in which you should inputyour answer: 1.2475e8.Useful formulae:NAAdensity (p) =V.Nawhere Avagadro's number Na= 6.022 x 1025 atoms/molNpQv= expkBT

Recall the given expression as follows NvNA=exp-QvKBTHere, equilibrium number of…

Answered: What is the equilibrium number of…

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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A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless- steel cylinder that measures 21.0 cm wide and 25.2 cm high. The maximum safe pressure inside the vessel has been measured to be 7.20 MPa, For a certain reaction the vessel may contain up to 1.45 kg of sulfur hexafluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits. temperature: °C
The Born-Haber process is, N2 (g) + 3 H2 (g) = 2 NH3 (g) has an equilibrium position when [N2] = 12.9 M, [H2] = 0.600 M and (NH3] =0.500 M. (a) What is the value of K? (b) If [N2] = 2.30 M, [H2] = 0.500 M and (NH3] =0.150 M, then are these concentrations at an equilibrium position? If not, then in which direction will a shift bring about equilibrium?
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HCl(g) 2NH4CI(S) at 340 °C is 4.00. (a) If the partial pressure of ammonia is PNH3 = 0.840 atm and solid ammonium chloride is present, what is the equilibrium partial pressure of hydrogen chloride at 340 °C? PHCI = (b) An excess of solid NH4Cl is added to a container filled with NH3 at 340 °C and a pressure of 1.34 atm. Calculate the pressures of NH3(9) and HCI(g) reached at equilibrium. PNH3 = atm PHCI = atm atm
A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder that measures 24.0 cm wide and 28.8 cm high. The maximum safe pressure inside the vessel has been measured to be 5.20 MPa. For a certain reaction the vessel may contain up to 0.658 kg of boron trifluoride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Be sure your answer has the correct number of significant digits.
The following system is at equilibrium in a closed vessel: 4 HCl(aq) + MnO2(s) ⇆ MnCl2(aq) + 2 Cl2(g) + 2 H2O(l) Various stresses are applied to the system as illustrated in the chart. Drag the appropriate label from the list below that indicates how the system responds to each stress. Each label can be used more than once.
Consider the following chemical reactions at equilibrium 1 A + 1 B = 3C K = 0.034 3C = 2 D + 1 E K= 100 What would be the value of the equilibrium constant for the following reaction: 2 D + 1 E = 1 A + 1 B
One application of adsorption on surfaces is to measure the ability of acti- vated charcoal to adsorb acid. (Activated charcoal, a form of treated carbon, is very porous and is used to adsorb impurities from water. Its use in aquar- iums typifies this behavior.) In a lab experiment, a student mixes a given amount of powdered charcoal into a series of acetic acid solutions. The acetic acid solutions have different initial concentrations. Some of the acid is ad- sorbed onto the charcoal. By taking aliquots after equilibrium is established, the student determines the change in acid concentration. Plot a Langmuir isotherm for the experimental data and determine the equilibrium constant for the adsorption. The experimental data are as follows: Original concentration (M) 0.7001 Change in concentration (M) 0.3694 0.1515 0.0437 0.0169 0.00665 0.00588 0.00553 0.00283 0.00153
When exposed to UV light, phosgene (COCL2) decomposes according to the reaction COCL2(g)->CO(g) + Cl2(g). All the air is removed from a flask. The flask is then filled with phosgene to a pressure of 2.8 atm and then exposed to UV light. If the temperature remains constant during the decomposition, what is the partial pressure of Cl2 (g) in the flask after the decomposition is complete, assuming 100% yield?
Using thermodynamic data to calculate K Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NH3(g) →>> 4 N₂H₁(g) + H2(g) Round your answer to 2 significant digits. K = П ☐ x10 ☑ 0/5 izabella ? ola 18 Ar 館
A mixture of 0.500 mol H2 and 0.500 mol I2 is placed in a 1.0-liter stainless steel container at 430 C. Calculate the equilibrium concentrations of H2, I2, and H1. The equilibrium constant for the reaction is 54.3 at that temperature.

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