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CHEM 6B Lecture Notes - Lecture 7: Phosphorus Trichloride, Phosphorus Pentachloride, Dinitrogen Tetroxide

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burgundyporpoise729

6 Apr 2018

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Department

Chemistry and Biochemistry

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Professor

Sandrine Bernoilles

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Document Summary

Are we at equilibrium: q = [no2]^2 / n2o4, 2. 00m^2 / 2. 00m = 2. 00m =/= . 20m. If pressure increased, equilibrium goes towards side with less gaseous moles: side with most gaseous moles gets too stressed, wants to go to side with less. Calculate the new pressures at eq once it has reestablished equilibrium: pcl3 + cl2 pcl5, 217 / 13. 2*13. 2 = kp = 1. 245, ptotal = 263 - 217 - 13. 2 = 32. 8 torr (cl2) Lewis acids and bases: lewis acid is an electron pair acceptor, lewis base is an electron pair donor, h2o + hcl h3o+ + cl , water goes from neutral to positive (has lost electrons) = lewis. Base: hcl goes from neutral to negative (has gained electrons) = lewis. [ ] = 10(-ph: 10 ^ -8. 22, 6. 03 x 10^-9 m, poh, numerical representation of the basicity of a solution, based on [oh-, ph + poh = 14.

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Related Questions

1. The value of Keq for the following reaction is 5.0 x 10-9
BaCO3(s) <--> Ba+2(aq) + CO32-(aq)

What statement is most correct about the equilibrium reactionmixture?
products dominate
reactants dominate
There is a reasonable mixture of reactants and products
only products exist.
only reactants exist.

2.For the reaction FeO(s) + CO(g) Fe(s) + CO2(g),
-the usual expression for the equilibrium constant is[Fe][CO2]/[FeO][CO]
-addition of CO2(g) will increase Kc.
-increasing the volume of an equilibrium mixture at constanttemperature will cause the number of moles of CO2 to increase asthe mixture re-equilibrates.
-adding more FeO to an equilibrium mixture will cause the number ofmoles of CO2 to increase as the system re-equilibrates.
-None of the above statements is true

3. Kc for the reaction F2(g) + Cl2(g)<--> 2 FCl(g) equals 125at a particular temperature. Suppose a system involving thisreaction is already at equilibrium and the concentrations of F2 andCl2 are found to be [F2] = 0.115 M and [Cl2] = 0.221 M. What is theconcentration of FCl in the system?
[FCl] = 1.78 M
[FCl] = 3.17 M
[FCl] = 2.54 x 10-2 M
[FCl] = 1.43 x 10-2 M
None of the above is within 5% of the correct answer

4. At high temperatures one mole of hydrogen gas reacts with onemole of bromine gas to form hydrogen bromide. At a giventemperature the equilibrium constant is 57.6. If at the sametemperature, a mixture of 4.67 x 10-3 M hydrogen gas, 2.14 x 10-3bromine gas, and 2.40 x 10-2 M hydrogen bromide gas is made,then
-the system is far from equilibrium and will shift to form morehydrogen gas.
-the system is far from equilibrium and will shift to form morehydrogen bromide gas.
-nothing can be deduced since we do not know whether the reactionis endothermic or exothermic.
-nothing can be deduced since we do not know whether theequilibrium constant is Kc or Kp.
-the system is at equilibrium.

5. Which one of the following equilibriums is least affected by achange in the volume of the system?
2 C(s) + O2(g) <--> 2 CO(g)
H2(g) + S(l) <---> H2S(g)
2 NO2(g)<--->N2O4(g)
H2O(l)<--->H2O(g)
2 NO(g) + Cl2(g)<-->2 NOCl(g)

carminetrout848

1. The value of Keq for the following reaction is 5.0 x 10-9
BaCO3(s) <--> Ba+2(aq) + CO32-(aq)

What statement is most correct about the equilibrium reactionmixture?
products dominate
reactants dominate
There is a reasonable mixture of reactants and products
only products exist.
only reactants exist.

2.For the reaction FeO(s) + CO(g) Fe(s) + CO2(g),
-the usual expression for the equilibrium constant is[Fe][CO2]/[FeO][CO]
-addition of CO2(g) will increase Kc.
-increasing the volume of an equilibrium mixture at constanttemperature will cause the number of moles of CO2 to increase asthe mixture re-equilibrates.
-adding more FeO to an equilibrium mixture will cause the number ofmoles of CO2 to increase as the system re-equilibrates.
-None of the above statements is true

3. Kc for the reaction F2(g) + Cl2(g)<--> 2 FCl(g) equals 125at a particular temperature. Suppose a system involving thisreaction is already at equilibrium and the concentrations of F2 andCl2 are found to be [F2] = 0.115 M and [Cl2] = 0.221 M. What is theconcentration of FCl in the system?
[FCl] = 1.78 M
[FCl] = 3.17 M
[FCl] = 2.54 x 10-2 M
[FCl] = 1.43 x 10-2 M
None of the above is within 5% of the correct answer

4. At high temperatures one mole of hydrogen gas reacts with onemole of bromine gas to form hydrogen bromide. At a giventemperature the equilibrium constant is 57.6. If at the sametemperature, a mixture of 4.67 x 10-3 M hydrogen gas, 2.14 x 10-3bromine gas, and 2.40 x 10-2 M hydrogen bromide gas is made,then
-the system is far from equilibrium and will shift to form morehydrogen gas.
-the system is far from equilibrium and will shift to form morehydrogen bromide gas.
-nothing can be deduced since we do not know whether the reactionis endothermic or exothermic.
-nothing can be deduced since we do not know whether theequilibrium constant is Kc or Kp.
-the system is at equilibrium.

5. Which one of the following equilibriums is least affected by achange in the volume of the system?
2 C(s) + O2(g) <--> 2 CO(g)
H2(g) + S(l) <---> H2S(g)
2 NO2(g)<--->N2O4(g)
H2O(l)<--->H2O(g)
2 NO(g) + Cl2(g)<-->2 NOCl(g)