Question

Please answer ALL parts OF LETTER F and show work/explain

LETTER F

5. Consider the following concentration table 4 NH3(g) 0.30 mol 702(g) 0.80 mol 〈=> 2N,04(g) + 6H20(g) I (initial moles) C (change) E (equilibrium moles) a) What are the values for each of the v;? b) Show that Σ v, Xi-0. c) Fill in the concentration table in terms of 5, the extent of reaction. d) According to your concentration table what are the minimum and maximum values that 5 can attain? (Hint: the equilibrium n, cannot be negative) e) Assume that the reaction is run at constant T and P. 1) If T and P are constant what is the relationship between the Pi and n? 2) Use your relationship of part 1) to convert each P, in Kp into an expression in n,. 3) Simplify the above expression by collecting into a product of two types of terms i) terms in n; and ii) constants. 4) Finally substitute the equilibrium moles into the simplified K of part 3). f) Assume that the reaction is run at constant T and V. 1) Express Kp in terms of the partial pressures P, remembering that K is unitless so that we divide each Pi by the standard pressure Po. This statement is also appropriate before 1) in part e) 2) If T and V are constant what is the relationship between the P, and n,? 3) Use your relationship of part 2) to convert each Pi in Kp into an expression in n, 4) Simplify the above expression by collecting into a product of two types of terms i) terms in nj and ii) constants. 5) Finally substitute the equilibrium moles into the simplified K of part 4).

Answer 1