please help within five minutes

SoccerBoss
Category:
Chemistry
Price: $5 USD

Question description

The equilibrium constant for HI decomposition at 500 °C is 5.8×10-3.
2HI(g) = H2(g) + I2(g)
At that temperature reactants and products are gaseous. (There is no change in the total number of moles, so Kc = Kp.)
A sample of 0.43 mol of HI is placed in a 1.00 L vessel which is then heated to 500 °C. When equilibrium is reached, what is the molar concentration of H2? (Give units).
 ============================================================================

Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction:

I-(aq) + I2(aq) I3-(aq) K = 710

For each of the following cases calculate the equilbrium ratio of [I3-] to [I2].

5.00×10-2 mol of I2 is added to 1.00 L of 5.00×10-1 M KI solution.

The solution above is diluted to 12.00 L.



Studypool has helped 1,244,100 students
Ask your homework questions. Receive quality answers!

Type your question here (or upload an image)

1829 tutors are online

Brown University





1271 Tutors

California Institute of Technology




2131 Tutors

Carnegie Mellon University




982 Tutors

Columbia University





1256 Tutors

Dartmouth University





2113 Tutors

Emory University





2279 Tutors

Harvard University





599 Tutors

Massachusetts Institute of Technology



2319 Tutors

New York University





1645 Tutors

Notre Dam University





1911 Tutors

Oklahoma University





2122 Tutors

Pennsylvania State University





932 Tutors

Princeton University





1211 Tutors

Stanford University





983 Tutors

University of California





1282 Tutors

Oxford University





123 Tutors

Yale University





2325 Tutors