Magnesium oxide (MgO) is an inorganic compound that occurs in nature as the mineral periclase, The atomic and ionic radi of Mg and O are Ru= 0.16 nm: Ru=0.078 nm Ro =0.06 nm; Ro =0.14nm. Calculate the Repulsive force between Mg" and O in Mgo at equilibrium. Given: 9= 1.6x10 1C Ke= 9*10°(V.m/C) Select one: O a. Fr-1.93*10 N Ob Fr=1.08*10N O c Fr1.08x10N O dgr=1.93-10 N

Magnesium oxide (MgO) is an inorganic compound that occurs in nature as the mineral periclase, The atomic and ionic radi of Mg and O are Ru= 0.16 nm: Ru=0.078 nm Ro =0.06 nm; Ro =0.14nm. Calculate the Repulsive force between Mg" and O in Mgo at equilibrium. Given: 9= 1.6x10 1C Ke= 910°(V.m/C) Select one: O a. Fr-1.9310 N Ob Fr=1.08*10N O c Fr1.08x10N O dgr=1.93-10 N

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

A student determines the value of the equilibrium constant to be 1.39x1025 for the following reaction. 2502(g) + O2(8)2S03(g) Based on this value of Keg: AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.84 moles of SO2(g) at standard conditions at 298K. AG° rxn kJ
8:41 1 4 7 +/- What is K for a reaction if AGº =86.0 kJ/mol at 25.0 °C? (R = 8.314 J/mol K) 2 5 8 Question 3 of 17 . 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
A student determines the value of the equilibrium constant to be 4.30×10-15 for the following reaction. 2CO₂(g) + 5H₂(g)C₂H₂(g) + 4H₂O(g) Based on this value of Keq: AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 1.72 moles of CO₂(g) at standard conditions at 298K. AGOrxn= kj Submit Answer than zero. Retry Entire Group 9 more group attempts remaining
Calculate AG° at 595 K for H20(g) + 1/2 O2(g) S H2O2(g) using the following data: H2(g) +O2(g) H2O2(g) K = 3.7 x 1037 at 595 K 2H2(g) + O2(g) 2H2O(g) K= 2.6 x 10° at 595 K AGO kJ/mol
1.4 4 (a) Calculate the value of Kc for the reaction: PCl5 (g) PCl3 (g) + Cl2 (g) ΔH = Positive Given that when 8.4 mol of PCl5 (g) is mixed with 1.8 mol of PCl3 (g) and allowed to come to equilibrium in a 10 dm3container the amount of PCl5 (g) at equilibrium is 7.2 mol. Kc =
Exactly 1.0 mol N,04 is placed in an empty 1.O-L container and allowed to reach equilibrium described by the equation N204(s) = 2NO,(g). If at equilibrium the N,04 is 28.0% dissociated, what is the value of the equilibrium constant, K. for the reaction under these conditions? 0.44 O 2.3 0.31 0.78 0.11
4G VOLTE O 76 14 4:58 7 February 2021 4:57 PM (ii) Calculate the lattice energy of Silica oxide (SiO2) from the data given below: Si (g) - Si (s) AH° = -454 kJ mol-1 S1A+ (E) + 4e" Si (3) AH° = -9949 kJ mol-1 20 (g) – 02 (3) AH° = -498 kJ mol-1 02 (3) 0 (g) + 2e AH° = -737 kj mol-1 Si (s) + 02 (3) → SiO2 (s) s14+ (6) - 202- (3) – SiO2 (s) AHf (SIO2)= -910.9 kj mol1 AH°lattice = ? Share Favourite Edit Delete More
Can you please show me how to do this? See image below....