C_10 H_2 (g) 2C_5 H_6 (g) Delta H degree = 77.0 kJ middot mol^-1 What temperatur

Question

C_10 H_2 (g) 2C_5 H_6 (g) Delta H degree = 77.0 kJ middot mol^-1 What temperature-pressure combination would maximize the concentration of C_5 H_6? At constant temperature and pressure, which will give the largest equilibrium constant? negative Delta H and positive Delta S negative Delta H and negative Delta S positive Delta H and positive Delta S positive Delta Hand negative Delta S What is the equilibrium constant for reaction 3? AgCl(s) Ag^+ (aq) + Cl^- (aq) K_sp = 1.8 Times 10^-10 Ag^+ (aq) + 2NH_3 (aq) [Ag(NH_3)_2] + (aq) K = 1.5 Times 10^7 AgCl(s) + 2 NH_3 (aq) [Ag(NH_3)_2] + (aq) + Cl^- (aq) 1.5 Times 10^7 3.7 Times 10^2 2.7 Times 10^-3 1.8 Times 10^-10

Explanation / Answer

I have a doubt in question 28, but here's answer for 27 and 29.

27. Let's suppose we have the following pressure and temperature:
P1 = 10 atm; P2 = 100 atm; P3 = 200 atm
T1 = 273 K; T2 = 298 K; T3 = 323 K)

Let's calculate concentration of one case, let's do first low -low
C1 = 10 / (0.0821*273) = 0.45 M

Now low-high pressure:
C = 100 / (0.0821*273) = 4.46 M

Now LEt's do T2-P2 (raising temperature)
C = 100 / (0.0821¨*298) = 4.09 M

As we can see if we raise temperature the concentration is lowering, so, let's try a higher pressure and lower temperatura:
C = 200 / (0.0821*273) = 8.92 M

So we can conclude that in order to get the maximum concentration, we need to increase pressure and decrease temperature.

29. As we are summing the two equations, the Kc is just multiplying the constants:
Kc = Ksp * Kf
Kc = 1.8x10-10 * 1.5x107
Kc = 2.7x10-3

Hope this helps

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