label Chemistry
account_circle Unassigned
schedule 1 Day
account_balance_wallet \$5

An equilibrium mixture, at 713°C in a 1500-mL container, involving the chemical system

N2(g) + 3H2(g)  2NH3(g)

is found to contain 5.27 g of N2, 0.339 g of H2, and 0.0477 g of NH3. Calculate the equilibrium constant (Keq expressed in terms of the molar concentrations) at the given temperature.

2,A 3.00-L vessel contained 9.10×10-2 mol of gaseous PCl3, 9.48×10-2 mol of gaseous PCl5, and 8.80×10-2 mol of Cl2 gas at equilibrium at 242°C.

Calculate the value of Keq for the reaction

PCl3(g) + Cl2(g)  PCl5(g)

May 5th, 2015

DATA:

Mass of N2= 5.27g = (0.1882 mol*1000)/1500 =0.1254M

Mass of H2=0.339g =(0.0188 mol*1000)/1500 =0.0125M

Mass of NH3= o.o477g = (0.0028 mol*1000)/1500=0.0018M

Keq =?

SOLUTION:

Keq = [NH3]2/[N2] [H2]3

By putting the molar concentrations of reactants and product in the above equation;

Keq = [.0018]2/[.1254] [.0125]3

= 13.22

May 5th, 2015

gonna send you the next solution.

May 5th, 2015

DATA:
mol of PCl3 = (9.10*10-2 mol*1000)/3000=0.0303M

Mole of PCl5 = (9.48*10-2 mol *1000)/3000=0.0316M

Mole of Cl2 = (8.80*10-2*1000)/3000= 0.0293M

Keq =?

SOLUTION:

Keq = [PCl5]/[PCl3] [Cl2]

= 0.0316/(0.0303) (0.0293)

Keq = 35.594

May 5th, 2015

DATA:

Mass of N2= 5.27g = (0.1882 mol*1000)/1500 =0.1254M

Mass of H2=0.339g =(0.1695 mol*1000)/1500 =0.113M

Mass of NH3= o.o477g = (0.0028 mol*1000)/1500=0.0018M

Keq =?

SOLUTION:

Keq = [NH3]2/[N2] [H2]3

By putting the molar concentrations of reactants and product in the above equation;

Keq = [.0018]2/[.1254] [0.113]3

= 0.0179

May 5th, 2015

...
May 5th, 2015
...
May 5th, 2015
Sep 24th, 2017
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle