Question

www .locatoriamente INTERACTIVE EXAMPLE Solving an Equilibrium Problem (Involving a Linear Equation in x) Chapter 54 Homework for Grade Question 1 1pl Question 2 1 pt Question 3 Question 4 pl The reaction CO(g) + H2O(g) + CO2(&)-H (8) has an equilibrium constant of 0.58 at 1000 °C. If 20.0-L mixture of CO and H.Ohas a concentration of each of 2.00x10"moll, what amount (in moles) of each species will be present when the mixture reaches equilibrium? mol CO Questions for mol H,O mol CO2 mol H Submit Hide Tutor Steps

Answer 1

                 CO(g) +    H₂O(g)      ↔ CO₂(g) +H₂(g), K_eq = 0.58

	CO(g)	H2O(g)	↔	CO2(g)	H2(g)
Initial	2.00 * 10-2	2.00 * 10-2		0	0
Change	-x	-x		+x	+x
Equilibrium	2.00 * 10-2 -x	2.00 * 10-2 -x		x	x

K_eq = [CO][H₂O] / [CO₂][H₂]

0.58 = (2.00 * 10^-2-x)² / x²

taking square root on both sides

0.762 = 0.02-x/x

0.762x =0.02-x

1.762x =0.02

X =0.02/1.762 =0.0113

So, at equilibrium

[CO]_eq = 0.02-0.0113 =0.0087 mol/L

[H₂O]_eq = 0.02-0.0113 =0.0087 mol/L

[CO₂]_eq =0.0113 mol/L

[H₂]_eq = 0.0113 mol/L

For 20 L mixture, the number of moles

[CO] = 20* 0.0087 =0.174 moles

[H₂O] = 20* 0.0087 = 0.174 moles

[CO₂] = 20 * 0.0113 = 0.226 moles

[H₂] = 20*0.0113 = 0.226 moles