Be sure to answer all parts. consider the following reaction: cd(s) + fe2+(aq) → cd2+(aq) + fe(s) e o (fe2+ / fe) = −0.4400 v, e o (cd2+ / cd) = −0.4000 v calculate the emf for this reaction at 298 k if [fe2+] = 0.80 m and [cd2+] = 0.010 m. e = v will the reaction occur spontaneously at these conditions? yes no cannot predict

EMF = -0.17 V

No

Explanation:  

For the reaction :

Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s)

we will be using the Nersnt equation to calculate Ecell:

Ecell =  Eº -0.0592 V/2 ln Q

where Q = ( Fe⁺² )/ (Cd²⁺)

and (Fe²⁺) and (Cd²) are the molar concentration of Fe²⁺ and Cd²⁺

Reduction

Fe²⁺ + 2e⁻  ⇒ Fe(s)      Eº red = -0.4400 V

Oxidation

Cd (s)   ⇒ Cd²⁺ + 2e⁻    Eº ox = +0.4000 V

Eºcell = Eox + Ered = 0.4000 V + (-0.4400 V) = -0. 0400 V

Ecell = Eº -0.0692 V/2 ln Q = -0.0400 V - 0.0592/2 ln ( 0.80/0.010 ) = -0.17V

No because Eºcell is negative and  ΔºG will be positive since

                               ΔºG  =  -nFEºcell

2b2t

explanation:

2b2t

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.