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prisoha [69]
3 years ago
12

iodid ion is oxidized to hypoiodite ion by permanganate what is the ratio of hydroxide ions to iodide ions in balanced equation

Chemistry
1 answer:
ad-work [718]3 years ago
4 0

<u>Answer:</u> The ratio of number of hydroxide ions to iodide ions is 2 : 1.

<u>Explanation:</u>

The chemical equation for the oxidation of iodide ion is oxidized to hypoiodite ion by permanganate follows:

2MnO_4^-+I^-+H_2O\rightarrow 2MnO_2(s)+IO_3^{-}+2OH^{-}

According to mole concept:

1 mole of a substance contains 6.022\times 10^{23} number of particles

Moles of iodide ions = 1 mole

Number of iodide ions = (1\times 6.022\times 10^{23}

Moles of hydroxide ions = 2 mole

Number of hydroxide ions = (2\times 6.022\times 10^{23}

Taking the ratio of number of hydroxide ions and number of iodide ions are as follows:

\frac{\text{Number of hydroxide ions}}{\text{Number of iodide ions}}=\frac{(2\times 6.022\times 10^{23})}{(1\times 6.022\times 10^{23})}\\\\\frac{\text{Number of hydroxide ions}}{\text{Number of iodide ions}}=\frac{2}{1}

Hence, the ratio of number of hydroxide ions to iodide ions is 2 : 1.

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The substance water always has a mass ratio of 11% H to 89% O. If 5.00g of a substance containing H and O was decomposed into .2
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Answer:

                    No the substance is not water.

Explanation:

                   The balance chemical equation for the decomposition of water is as follow;

                                           2 H₂O = 2 H₂ + O₂

Step 1: <u>Calculate moles of H₂O;</u>

               Moles  =  Mass / M.Mass

               Moles  =  5.0 g / 18.01 g/mol

               Moles  =  0.277 moles of H₂O

Step 2: <u>Calculate Moles of O₂ and H₂ produced by 0.277 moles of H₂O:</u>

According to equation,

                        2 moles of H₂O produced  =  1 mole of O₂

So,

                  0.277 moles of H₂O will produce  =  X moles of O₂

Solving for X,

                     X =  0.277 mol × 1 mol / 2 mol

                     X =  0.138 moles of O₂

Also,

According to equation,

                        2 moles of H₂O produced  =  2 mole of H₂

So,

                  0.277 moles of H₂O will produce  =  X moles of H₂

Solving for X,

                     X =  0.277 mol × 2 mol / 2 mol

                     X =  0.227 moles of H₂

Step 3: <u>Calculate Mass of O₂ and H₂ as;</u>

For O₂:

                 Mass  =  Moles × M.Mass

                 Mass  =  0.138 mol × 31.99 g/mol

                 Mass  =  4.44 g of O₂

For H₂:

                 Mass  =  Moles × M.Mass

                 Mass  =  0.227 mol × 2.01 g/mol

                 Mass  =  0.559 g of H₂

Conclusion:

                   From conclusion it is proved that the amount of H₂ produced by decomposition of 5 g of water should be 0.559 g while in statement it is less i.e. 0.290 g.

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