Using the standerd half-cell potential listed, calculate the equilibrium constant for the reaction : `Co(s)+2H^(+)(aq)toCo^(2+)(aq)+H_(2)(g)" at 298 K"` `Co^(2+)(aq)+2e^(-)toCo(s) E^(@)=-0.277 V`A. `2.3xx10^(9)`B. `4.8xx10^(4)`C. `4.8xx10^(7)`D. `4.8xx10^(11)`

Using the standerd half-cell potential listed, calculate the equilibri

1.	Using the standerd half-cell potential listed, calculate the equilibrium constant for the reaction : `Co(s)+2H^(+)(aq)toCo^(2+)(aq)+H_(2)(g)" at 298 K"` `Co^(2+)(aq)+2e^(-)toCo(s) E^(@)=-0.277 V`A. `2.3xx10^(9)`B. `4.8xx10^(4)`C. `4.8xx10^(7)`D. `4.8xx10^(11)`
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What are elementary reactions ?

Using the standerd half-cell potential listed, calculate the equilibrium constant for the reaction : `Co(s)+2H^(+)(aq)toCo^(2+)(aq)+H_(2)(g)" at 298 K"` `Co^(2+)(aq)+2e^(-)toCo(s) E^(@)=-0.277 V`A. `2.3xx10^(9)`B. `4.8xx10^(4)`C. `4.8xx10^(7)`D. `4.8xx10^(11)`

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