Redox equations are often long and difficult to balance by inspection. Using oxi

Question

Redox equations are often long and difficult to balance by inspection. Using oxidation states and half-reactions you can more easily balance a redox reaction. Balance the following equation:_K_2CrO_4 + Na_2SO_3 + HC1rightarrowKC1 + Na_2SO_4 + CrCl_3 + H_2O Generally coefficients of 1 are omitted from balanced chemical equations. When entering your answer, include coefficients of 1 as required for grading purposes. Enter the coefficients for each compound, separated by commas, in the order in which they appear in the equation(e.g., 1, 2, 3, 4, 5, 6, 7). In the process of oxidizing T^- to T_2, SO_4^2- is reduced to SO_2. How many moles of SO_2 are produced in the formation of one mole of I_2 ?

Explanation / Answer

Answer:

PartA:

2 K2CrO4 + 3 Na2SO3 + 10 HCl = 4 KCl + 3Na2SO4 + 2 CrCl3 + 5 H2OO.

PartB:

2 I- +SO4 2- = I2 + SO2 + O2.

So, one mole of SO2 produced for formation of one of I2.

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