The reaction A(g) + 2B(g) c(g) was allowed to come to equilibrium. Calculate K_e

Question

The reaction A(g) + 2B(g) c(g) was allowed to come to equilibrium. Calculate K_e for this reaction. Equilibrium is established for the reaction 2X(s) + Y(g) 2Z(g) at 500K. K_e = 100. determine the concentration of Z in equilibrium with 0.2 mot times and 0.50 M Y at 500K. Consider the reaction N_2(g) + O_2(g) 2NO(g), for which K_c = 0.10 at 2,000 degree C. Starting with initial concentrations of 0.040 M of N_2 and 0.040 M of O_2. determine the equilibrium concentration of NO. Sodium carbonate. Na_2CO_3(s), can be prepared by heating sodium bicarbonate, NaHCO_3(s) as shown below. If a sample of NaHCO_3 is placed in an evacuated flask and allowed to achieve equilibrium at 100 degree C. what will the total gas pressure be? Which of the following does not fit the definition of a Bronsted Acid? Which of the following does not fit the definition of a Brensted Base?

Explanation / Answer

Too many questions in the same post. I will answer only 3 questions. The other questions post them in another question thread and per separate (no more of 2 or 3 questions per post).

Question 11.

[B] = 1.8 / 5 = 0.36 M
[A] = 1 / 5 = 0.20 M

r: A + 2B -------> C
i. 1 1.8 0
e. 1-x 1.8-2x x

Now, we know that at the equilibrium moles of B = 1 mol which means that:
1 = 1.8-2x ---> x = 1.8-1/2 = 0.4

therefore the moles of A and C are:
moles A = 1-0.4 = 0.6 moles
moles C = 0.4 moles

Kc = 0.4/5 / (0.6/5) * (1/5)2
Kc = 16.67

Question 12.
Kc = Kp / (RT)dn
dn = 2-1 = 1
Kc = 1.47 / 0.082 * (727+273)
Kc = 0.0224

Question 13 is the same as question 12, but changing values of Kp, T and dn.

Question 16.
The only compounds we need to take account here are the compounds in the gaseous state which are CO2 and H2O. If we assume that both of them exerts the same pressure then:
Kp = pCO2*pH2O
0.23 = x2
x = 0.48 atm --Z Option D.

Hope this helps

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