Determine the whole number mole ratio of two reactants given volume of OCl and S

Question

Determine the whole number mole ratio of two reactants given volume of OCl and S2O3 and temperature change?

Which solution is the limiting reactant?

Find the actual balanced equaition for the reaction OCl- and S2O3. Does the mole ratio determined match the actual reaction equations coeffiecents for the two reactants? explain if your mole ratios do not match.

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so far i think the whole number ratio of the two reactants is 4OCl + 1S2O3, i think this because the greatest temp change was at 40mL of OCl and 10mL of S2O3, but not sure if its right and the rest im not sure how to even start

Volume OCl- (mL) Volume S2O3 (mL) Temperature Change (C) 10.0 40.0 3.6 25.0 25.0 9.8 40.0 10.0 15.8 45.0 5.0 13.4 47.0 3.0 7.3 49.0 1.0

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Explanation / Answer

4 OCl{-} + S2O3{-2} + 2 OH{-} = 2 SO4{-2} + 4 Cl{-} + H2O

This is the actual balanced reaction equation

and yes you are right the it is due to the greatest temperture difference in the case 40 ml of OCl{-} and 10 ml of  S2O3{-2}

Because according to collision theory the two reactant should effectively collide with each other to cross the energy barrior condition for which they require greater heat supplied to it and the in the above case the temperture difference is maximum so this is the favourable reaction

If the moles ratio doesnot match it is fractional order reaction

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