Chemistry- Reaction kinetics, Water/equilibrium?
A 1.00 mol kg-1 sloution of H2SO4 in water boils at 101.380 degrees celsius. {Kbp (H2O)=0.51 degrees celsius kg mol-1}
calculate the concentration of particles in this solution?
What I did was;
changeIn T= K x m
observed; 101.38-100= 1.38 C
calculated= 0.51 x 1 x i=0.51 x i
Then 1.38/0.51= i = 2.7
I don't understand how to calculate the concentration.
Also, if my above working out is correct, does that mean that H2SO4 mainly exists as 2H+, SO4 2- ? I am confused as I thought that H2SO4 is a strong acid and so it should exist as H+, HSO4 -
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First order reaction of N2O4 to form 2 mol of NO2 has rate constant k=0.023 min-1. How long will it take the initial concentration of N2O4 to decrease to 10% of the original value?
a)600s, b) 100 min c)43.5s d)43.5 min e) 435 min
I am confused as to how to do this question;
I'm unsure of how to do this question as I can only think of rate=k x [NO2]
How to do this question?
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Enthalpy is a very useful thermodynamic quantity because it relates to measurements made in a system which is:
a)isolated
b)at constant pressure
c)constant temperature
d)spontaneous