Consider the following cell:
`2Fe(s)+O_2(g)+4H^+(aq)rarr2Fe^(3+)(aq)+2H_2O(l)`
`E_(cell)^@=1.67V`. When `[Fe^(2+)]=1xx10^-3M`, `p(O_2)=0.1atm` e.m.f of the cell is 1.57V. Calculate the pH of the solution.

Balance the following equation : Fe + O2 → Fe2O3

Complete the following chemical equation : MnO_4^(-)(aq) + S_2O_3^(2-)(aq)+ H_2O (l) rarr

Complete the following chemical equation : Cr_2O_7^(2-) (aq)+ Fe^(2+) (aq)+ H^(+) (aq)rarr

The cell in which the following reaction occurs: 2Fe^(3+)(aq)+2I^(-)(aq)rarr2Fe^(2+)(aq)+I_2(s) has E_(cell)^o=0.236 V at 298 K. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Write Nernst equation for the following cell reaction: 2Al(s)+3Fe^(2+)(aq)rarr2Al^(3+)(aq)+3Fe(s)

Complete the following chemical reaction equations . Cr_2O_7^(2-) (aq) + Fe^(2+) (aq) + H^+ (aq) to

Balnce the following equations: CH_4 (g) + O_2 (g) rarr CO_2 (g) + H_2O(g) Al(s) + HCl (aq) rarr AlCl_3 (aq) H_2 (g)

The e.m.f of the cell Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1xx10^-xM)|Cu is 2.651 V. The standard e.m.f of the cell is 2.71 V. the value of x is

The decomposition of hydrogen peroxide in the presence of iodide ion has been found to be first order in H_2O_2 : 2H_2O_2 (aq) overset(1^(-)(aq))(rarr) 2H_2O(l) + O_2 (g) . The rate constant has been found to be 1.01 xx10^(-2) " min"^(-1) : (a) Calculate the rate of reaction when [H_2O_2] = 0.4" mol lit"^(-1) . (b) What concentration of [H_2O_2] would give a rate of 1.12 xx 10^(-2)" mol lit"^(-1)" min"^(-1) ?

Calcualate the Delta_rG for the reaction: Mg(s)+Cu^(2+)(aq)rarrMg^(2+)(aq)+Cu(s) Given: E_(cell)^@=+2.71V, 1F=96500C mol^-1