If 2.5 x 10-4 moles of Na2S2O3 are present in the starting solution, how many moles of H2O2 are used up by the time the solution turns blue? (See equations 6 and 7) If the total volume of the solution is 100 mL and the reaction requires 600 seconds, what is the value of the average rate of reaction ( -Δ[H2O2]/Dt)? Show units. H2O2+ 2 I−+ 2 H+→I2+ 2 H2O (6) 2 S2O3 2-+ I2 →2 I−+ S4O62− (7) I don't know if you can help me with this equation at all but any help would be appreciated!!
If 2.5 x 10-4 moles of Na2S2O3 are present in the starting solution, how many moles of H2O2 are used up by the time the solution turns blue? (See equations 6 and 7) If the total volume of the solution is 100 mL and the reaction requires 600 seconds, what is the value of the average
H2O2+ 2 I−+ 2 H+→I2+ 2 H2O (6)
2 S2O3 2-+ I2 →2 I−+ S4O62− (7)
I don't know if you can help me with this equation at all but any help would be appreciated!!
Given : mole of Na2S2O3 = 2.5×10^-4
Volume of solution = 100 ml
Difference in time = 600 sec.
To find : mole of H2O2 required and average rate of reaction of H2O2
Solution : As we know that, mole of any reactant depends upon the the mole of given reactants. Mole of any substance is the ratio of mass and molar mass of substance.
Mole =mass /molar mass
Generally rate of reactants in a reaction is negative which show the rate of consumption of reactants and rare of product is positive which shoe rate of formation of products.
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