A chemist is studying the following equilibrium: 2Pb(NO3)2 (s) <--> 2PbO (s) + 4

Question

A chemist is studying the following equilibrium:
2Pb(NO3)2 (s) <--> 2PbO (s) + 4NO2(g) + O2 (g)
He starts out with 10 g of Pb(NO3)2 and, at equilibrium, has 2.02 gof PbO. The concentrations of NO2 and O2 at equilibrium are 0.25 M and0.019 M, respectively. What is the value of theequilibrium constant?

Please explain the best you can.
Misa :)

2Pb(NO3)2 (s) <--> 2PbO (s) + 4NO2(g) + O2 (g)
He starts out with 10 g of Pb(NO3)2 and, at equilibrium, has 2.02 gof PbO. The concentrations of NO2 and O2 at equilibrium are 0.25 M and0.019 M, respectively. What is the value of theequilibrium constant?

Please explain the best you can.
Misa :)

Explanation / Answer

   We Know that :        The given Reaction is:         2Pb(NO3)2 (s) <--> 2PbO (s) + 4NO2 (g) + O2(g)         Kc = [ NO2 ]4 [ O2]           For the calculation of equilibrium constant we usually take theconcentration of solids                                                        as unity.               = [ 0.25 M ]4 [ 0.019 M ]                = 0.00007421875

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