The decomposition of hydrogen peroxide was studied and thefollowing data was obt

Question

The decomposition of hydrogen peroxide was studied and thefollowing data was obtained:

Mols/liter Time (sec)
1.000        0.000
0.910        120.0
0.780        300.0
0.590        600.0
0.370        1200.0
0.220        1800.0
0.130        2400.0
0.082        3000.0
0.0500       3600.0

c. Write a general rate law for this reaction
d. determine the order of reaction by rate law comparison
e. using the order of reaction and the rate law, calculate kwith units
f. determine the rate of reaction at a concentration of .450mols/liter, using the k and the rate law derived in the previousstep

Help.. can someone show me how to do these. They all relate to oneanother! help!

Explanation / Answer

We Know that :    Decomposition of hydrogen -peroxide in thepresence of dilute base follows first-order Reaction.         H2O2 ------> H2O   + 1/ 2 O2           Rate = K [ H2O2]0          Order of theReaction is 0.          Rate = -dC / dt                   = - (0.910 - 1.00) / 120 - 0                    = 75 x 10-5 Mol / L -s      K =   Rate / concentration of [ H2O2 ]           = 75 x 10-5 Mol / L -s / 1.00            = 75 x 10-5 Mol / L -s          As theabove Reaction is zero - order reaction which doesn't depends onthe concentration of the Reactant so the          Rate of theequation for the concentration 0.450 Mol / L is 75 x10-5 Mol / L -s              

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