For the reaction n2(g) + 3 h2(g) = 2 nh3(g), kp = 0.0489 at 256˚c. for parts a through d, assume that the reaction is at this temperature. c) a third equilibrium mixture contains 0.0100 mol/l of n2 and 0.0300 mol/l of nh3.what is the concentration of h2 in this mixture? d) a fourth equilibrium mixture contains equal concentrations of all three chemicals. what is the pressure of each substance in this mixture? me on c & d by 11/25 11pm !

Explanation:

c) Concentration of in this mixture

:

=(gaseous mole on product side)-(gaseous mole on reactant side)=2-4=-2

R = 8.314 J/mol K

T = 256 °C = 256+273 = 529 K

The concentration of hydrogen gas is 218.62 mol/L

d)A fourth equilibrium mixture contains equal concentrations of all three chemicals

x =

According ideal gas equation:

PV=nRT

Total pressure,P = 0.1343 atm

Partial pressure of nitrogen gas

Partial pressure of hydrogen gas

Partial pressure of ammonia gas

h let me think

quartz

explanation: