Chemistry Questions?

Question

39. The equilibrium system 2H2S(g) <-> 2H2(g)+S2(g) at a given temp was found to contain 1.0 mol H2S 2.0 mol H2 and 0.40 mol S2 in a 2.0 L containter the equilibrium constant is ???

40. Given the equilibrium S)2Cl2(g) <-> So2(g)+Cl2(g) delta h =+67 kJ the concentration of SO2 at equilibrium will be increased by???

41. In which of the following reaction does a decrease in the volume of the reaction vessel at constant temperature favor formation of the products???
a. H2(g) +I2(g)<-> 2HI(g)
b. MgCO3(s)<-> MgO(s) <-> MgO(s)+CO2(g)
c. NO2(g)+CO(g)<-> NO(g)+CO2(g)
d.2H2(g)+O2(g)<-> 2H2O(g)
e. 2O3(g)<->3O2(g)

42. For a specific reaction which of the statements can be made about an equilibrium contant?
a. it always remains the same
b. it inc. when the concentration of one of the products is inc.
c. it changes with changes in the temp
d. it inc. when the concentration of one of the reactants is inc.
e. it can be changed by the addition of a catalyst

Answer 1

Hello Kristin I am happy to help you another time!
39.
[H2S ] = 1.0 / 2.0 = 0.5 M
[H2] = 2.0 ] / 2.0 = 1.0 M
[S2 ] = 0.40 / 2.0 = 0.20 M
K = [H2]^2[S2] / [H2S]^2 = 1^2 x 0.20 / (0.5)^2 = 0.80

40.
DeltaH > 0 It is an endothermic reaction : if the temperature will decrease the concentration of products ( SO2 and Cl2 ) will increase

41.
d

42.
c

Answer 2

39. = [s2][h2]^2 / [h2s]^2

= .4/2 x 1 / .25

= 0.2 / 0.25
= 0.8

40. extracting some cl2(g) from the system.
adding to the product on the left of equatio (cant tell wat it is sorry)
or cooling the system
will all increase concentraion of so2


41. d.
because there are less gas particles on the right of the equation

42. c.
equilibrium constants are always constant for a given temperature.

Answer 3

It isn't worth the time to answer all the questions to get "points". Give us a break!!