At a particular temperature assume that the equilibriumconstant for the reaction

Question

At a particular temperature assume that the equilibriumconstant for the reaction:

H2(g) + F2(g) <==>2HF(g)

is K = 100.0. A reaction mixture in a 10.00 liter flask contains4.1 moles each of hydrogen and fluorine gases plus 3.4 moles of HF.What will be the concentration of hydrogen when this mixturereaches equilibrium? I've tried solving this question a dozen times and still can'tget the right answer. I've tried solving it assuming the reactiongoes forward(to the right) and tried solving it going backwards(tothe left). Nothing seems to work. At a particular temperature assume that the equilibriumconstant for the reaction:

H2(g) + F2(g) <==>2HF(g)

is K = 100.0. A reaction mixture in a 10.00 liter flask contains4.1 moles each of hydrogen and fluorine gases plus 3.4 moles of HF.What will be the concentration of hydrogen when this mixturereaches equilibrium? I've tried solving this question a dozen times and still can'tget the right answer. I've tried solving it assuming the reactiongoes forward(to the right) and tried solving it going backwards(tothe left). Nothing seems to work.

Explanation / Answer

Simply finout molarity of each one and then assume any ofdirection then write               c1(1-x)    c2(1-x)       c3(1+2x) findout value of x as k=    [c3(1+2x)*c3(1+2x)] /   (c1c2(1-x*x))

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