equilibrium
what is the equilibrium expression for the following equation
2 H2 (g) + 2 FeO(s) -> 2 Fe(s) + 2 H2O(g)
Kc= [H2O]2/[H2]2
What is the pH of a 0.0235 M HCl solution?
1.629
Consider the equilibrium reaction: N2O4(g) ⇌ 2NO2(g)
Which of the following correctly describes the relationship between Kc and Kp for the reaction?
Kp=Kc(RT)
what is the periodic table trend for acid strength?
as you move to the right and down the periodic table, acid strength increases
when delta g is negative
write the equilibrium expression for the following equation
3 H2 (g) + N2(g) ⇌ 2 NH3 (g)
[NH3]2/[H2]3[N2]
What is the pOH of a 0.0235 M HCl solution?
12.371
For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the
I2 concentration to increase?
2 NOI(g) ⇌ 2 NO(g) + I2(g)
add more NOI
Arrange the following in order of increasing acid strength: H2O, H2S, H2Se, H2Te
H2O < H2S < H2Se < H2Te
For some reaction, delta H is negative and delta S is positive. is the reaction spontaneous or non spontaneous?
spontaneous
The equilibrium 2 NO(g) + Cl2 (g) ⇌ 2 NOCl2 (g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl2, respectively. Calculate the value of Kp for this reaction at 500 K
51
What is the pH of a 6.50 x 10-3 M KOH solution?
11.813
Which of the following statements is correct if delta G° < 0?
a. K is greater than one, and the reaction favors reactants.
b. K is greater than one, and the reaction favors products
c. K is less than one, and the reaction favors reactants.
d. K is less than one, and the reaction favors products.
B
Arrange the following in order of increasing acid strength, HClO4 , HBrO2 , HIO2 , HClO3
HIO2 < HBrO2 < HClO3 < HClO4
what is the gibbs free energy equation?
delta g = delta H - TdeltaS
In which of these gas-phase equilibria is the yiel d of products increased by increasing the total pressure
on the reaction mixture?
a. CO(g) + H2O(g) ⇌ CO2 (g) + H2(g)
b. 2 NO(g) + Cl2 (g) ⇌ 2 NOCl(g)
c. 2 SO3 (g) ⇌ 2 SO2 (g) + O2 (g)
d. C(s) + CO2 (g) ⇌ 2 CO(g)
B
What is the pH of a 0.052 M NaOH solution?
12.72
Consider the following equilibrium process:
PCl5 (g) ⇌ PCl3(g) + Cl2 (g)
delta Hº = 92.5 kJ/mol.
Which one of the following statements is correct?
a. Kp at 800 K is smaller than Kp at 1,200 K.
b. Kp at 1,200 K is smaller than Kp at 800 K.
c. Temperature does not affect Kp .
d. Kp depends on total pressure as well as temperature.
A
what is the conjugate acid of HPO42-?
The value of K for a chemical reaction is 2.3 × 10-4 . Calculate deltaGºrxn at 25 ºC. Is the reaction spontaneous at this temperature?
no
given
HF(aq) ⇌ H+(aq) + F-(aq) K1 = 6.8 × 10-4
H2C2O4 (aq) ⇌ 2 H+(aq) + C2O42-(aq) K2 = 3.8 × 10-6
find k for the following expression in terms of k1 and k2
C2O42-(aq) + 2 HF(aq) ⇌ 2 F-(aq) + H2C2O4 (aq)
[K1]2/[K2]
What is the pH of a 0.0035 M BaOH2 solution?
11.85
for 3H2(g)+ N2(g) -> 2NH3(g), and Kc=6x10-2, if 0.25 M H2 and 0.05 NH3 are present at equilibrium, what is the equilibrium concentration of NH2?
2.7 M
what is the conjugate base of HCO3-
CO32-
Calculate K at 25 ºC given that deltaGºrxn = -25.3 kJ/mol. Is the reaction spontaneous at this temperature?
yes