In: Chemistry
consider the following unbalanced redox reaction Cr2O2−7(aq)+Cu(s)→Cr3+(aq)+Cu2+(aq)
a)Balance the equation: αCr2O2−7(aq)+βH+(aq)+γCu(s)→δCr3+(aq)+ϵH2O(l)+κCu2+(aq)
b)Determine the volume of a 0.950 M K2Cr2O7 solution required to completely react with 5.40 g of Cu.
(a) Balanced Chemial Equation:
Cr2O72- (aq) + 14 H+ + 3Cu 2Cr3+ + 3 Cu2+ + 7H2O
That means = 1, = 14, = 3, = 2, = 7, = 3
It is a redox reaction. First calculate the oxidation state of the
species included in the reaction. Oxidation state of
Cr in Cr2O72- is +6. Cu is in zero
oxidation state on reactant side. Therefore now student can write
two separate reaction.
Reduction half reaction: Cr2O72- (aq) Cr3+ (Gain of electrons)
Oxidation half reaction: Cu (s) Cu2+ (aq) (loss of electrons)
Now balance the coefficients in both reactions as follow:
Cr2O72- (aq) 2Cr3+
Cu (s) Cu2+ (aq)
Next balance the oxygen by using H2O
Cr2O72- (aq) 2Cr3+ + 7H2O
Next balance H with the help of H+
Cr2O72- + 14 H+(aq) 2Cr3+ + 7H2O
Next balance positive charges with the help of e-
Cr2O72- + 14 H+(aq) + 6e- 2Cr3+ + 7H2O
Cu (s) Cu2+ (aq) + 2e-
Now to cancel electrons multiply both equation with a whole number. In this case, mutiply first equation with 1st and 2nd equation with 3 and then add both equation to get final balanced equation.
Cr2O72- + 14 H+(aq) + 6e- 2Cr3+ + 7H2O
3Cu (s) 3Cu2+ (aq) + 6e-
On adding the above two equations 6 electrons will cancel out on both sides and we will get final equation.
Cr2O72- (aq) + 14 H+ + 3Cu 2Cr3+ + 3 Cu2+ + 7H2O
(b) First convert g of Cu into moles
No. of moles = m/M (m = mass given in grams and M =molecular mass of Cu)
= 5.40/63.54 = 0.0849 moles
From the balanced chemical equation student can conclude that
1 mole of K2Cr2O7 = 3 moles of Cu
Moles of K2Cr2O7 = 0.0849/ 3 = 0.0283
Molarity = no of moles / Volume of solution (in L)
Put the value of molarity and number of moles in the formula and calculate the volume
0.950 = 0.0283 / Volume
Volume = 0.0283/ 0.950 = 0.0297L = 29.7 mL
Therefore volume needed comes out to be = 29.7 mL