Justify the following reactions are redox reaction :
`Fe_(2)O _ 3` (s) + 3CO(g) ` rarr ` 2Fe(s) + 2 CO_ 2` (g)

Justify the following reactions are redox reactions : 2K(s) + F_2 (g) rarr 2K^+F^- (s)

Justify the following reactions are redox reaction : CuO(s) + H_2 (g) rarr Cu (s) + H_2O(g)

Justify the following reactions are redox rections : 4NH_3(g) + 5O_2(g) rarr 4NO(g) + 6H_2O (g)

Justify the following reactions are redox reactions : 4BCl_3(g) + 3LiAIH_4 (s) rarr 2B_2H_6 (g) + 3LiCl(s) + 3AICl_3 (s)

Determine DeltaS_(Total) and decide whether the following reaction is spontaneous at 298 K. Fe_2O_(3(s))+ 3CO_((g)) rarr 2Fe_(s) + 3CO_(2(g)) DeltaH^@ =- 24.8 kj, DeltaS^@ = + 15 JK^(-1)

Justify the following raection as redox reaction. 2 Na(s) + S(s) rarr Na_2 S(s) Find out the oxidizing and reducing agents.

Balance the following redox reactions by ion- electron method: H_2O_2 (aq) + Fe^(2+) (aq) rarr Fe^(3+) (aq) + H_2O (l) (in acidic solution)

Balanced the following reactions by oxidation number method H_2SO_4 (aq) + C(s) rarr CO_2 (g) + SO_2 (g) + H_2O(l) (acidic)

The standard reduction potentials at 25^(@)C for the following half reactions are given against each: Zn^(2+) (a.q) + 2e^(-) rarr Zn (s) : " " - 0.762 Cr^(3+) (a.q) 3e^(-) rarr Cr (s) , " " - 0.740 2H^(+) + 2e^(-) rarr H_(2) (g), " " 0.00 Fe^(3+) + e^(-) rarr Fe^(2+) , " " 0.77 Which is the strongest reducing agent?

Balance the following redox reactions by ion- electron method: Cr_2O_7^(2-) (aq) + SO_2 (g) rarr Cr^(3+) (aq) + SO_4^(2-) (aq) (in acidic solution)