Question

please any one balance this equation: CuSCN + KIO3 + HCl === CuSO4 + KCl + HCN + ICI + H2O

Answer 1

Answer:

Instructions on balancing chemical equations:

Enter an equation of a chemical reaction and click 'Balance'. The answer will appear below

Always use the upper case for the first character in the element name and the lower case for the second character. Examples: Fe, Au, Co, Br, C, O, N, F. Compare: Co - cobalt and CO - carbon monoxide

To enter an electron into a chemical equation use {-} or e

To enter an ion specify charge after the compound in curly brackets: {+3} or {3+} or {3}.

Example: Fe{3+} + I{-} = Fe{2+} + I2

Substitute immutable groups in chemical compounds to avoid ambiguity.

For instance equation C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced,

but PhC2H5 + O2 = PhOH + CO2 + H2O will

Compound states [like (s) (aq) or (g)] are not required.

If you do not know what products are enter reagents only and click 'Balance'. In many cases a complete equation will be suggested.

Reaction stoichiometry could be computed for a balanced equation. Enter either the number of moles or weight for one of the compounds to compute the rest.

Limiting reagent can be computed for a balanced equation by entering the number of moles or weight for all reagents.

Answer 2

Answer:

Step 1. Write down the unbalanced equation ('skeleton equation') of the chemical reaction. All reactants and products must be known. For a better result write the reaction in ionic form.

CuSCN + KIO3 + HCl → CuSO4 + KCl + HCN + ICl + H2O

Step 2. Separate the redox reaction into half-reactions. A redox reaction is nothing but both oxidation and reduction reactions taking place simultaneously.

a) Assign oxidation numbers for each atom in the equation. Oxidation number (also called oxidation state) is a measure of the degree of oxidation of an atom in a substance (see: Rules for assigning oxidation numbers).

Cu+1S-2C+4N-3 + K+1I+5O-23 + H+1Cl-1 → Cu+2S+6O-24 + K+1Cl-1 + H+1C+2N-3 + I+1Cl-1 + H+12O-2

b) Identify and write out all redox couples in reaction. Identify which reactants are being oxidized (the oxidation number increases when it reacts) and which are being reduced (the oxidation number goes down).

O:Cu+1S-2C+4N-3 → Cu+2S+6O-24(Cu)

Cu+1S-2C+4N-3 → Cu+2S+6O-24(S)

R:Cu+1S-2C+4N-3 → H+1C+2N-3(C)

K+1I+5O-23 → I+1Cl-1(I)

c) Combine these redox couples into two half-reactions: one for the oxidation, and one for the reduction (see: Divide the redox reaction into two half-reactions). It is necessary to combine all redox pairs with species containing several different redox atoms into one equation. Before combining the two reactions it is neccesary to ensure that the same coeficients are in front of both such molecules.

O:Cu+1S-2C+4N-3 → Cu+2S+6O-24 + H+1C+2N-3

R:K+1I+5O-23 → I+1Cl