Can anyone provide solutions and explanations to below questions? thank you!
1. a hypothetical equilibrium reaction conducted in an inert chamber at an atmospheric pressure is given as follows:
2A (aq) <--->B(aq) + C(aq) + 100kJ
a) write the expression for the equilibrium constant.
b) the equilibrium constant Keq is found to be 150. briefly explain what the numerical value represents in terms of the extent of the conversion of reactants to products.
c) given that Keq is 150, determine the equilibrium concentration of each reactant and product.
d) examined what happens to the equilibrium position when the product C is drawn from the reactant mixture for further processing.
2.
a) Consider the following reaction:
2NO (g) + 2H2(g) ---> N2(g) + 2H2O (g)
the reaction is first order in H2, and second order in NO. When [NO] = 0.035M, and [H2] = 0.015M, the rate of disappearance of NO at 1000K is 1.1025M/s.
(i) write the rate law for the reaction.
(ii) demonstrate that the value of the rate constant is 6.0 x 10^4. define the SI unit for the rate constant.
(iii) if the concentration of NO is now doubled, solve for the rate of appearance of N2.
b) list three natural emissions from unstable radioactive nuclei. compare and contrast them in terms of charges and penetrating power (i.e low, medium, high).