Question

In: Chemistry

22. For which one of the following reactions is Kp equal to Kc? a. 4NH3(g) +...

22. For which one of the following reactions is Kp equal to Kc?

a. 4NH3(g) + 5O2(g)   4NO(g) + 6H2O(g)                              

b. C(s) + CO2(g)   2CO(g)

c. 6CO2(g) + 6H2O(l)   C6H12O6(s) + 6O2(g)

d. CaCO3(s)   CaO(s) + CO2(g)

e. H2O(g) + C(s)   H2(g) + CO(g)

Solutions

Expert Solution

Ans. Using the equation-

Kp = Kc (RT)dn                       - equation 1

            Where,

            Kp = equilibrium constant in term of partial pressure

            Kc = equilibrium constant in term of concentration

            R = Universal gas constant= 0.0821 atm L mol-1K-1

            T = temperature in kelvin

                dn = total number of moles of product- total number of moles of reactants

Option A. dn = (6 + 4) – (4 + 5) = 1

Option B. dn = (2) – (1 + 1) = 0

Option C. dn = (1 + 1) – (1) = 1

Option D. dn = (1 + 1) – (1 + 1) = 0

Now, when dn = 0

            Kp = Kc (RT)0

            Or, Kp = Kc x 1                                    ; (X)0 = 1; so (RT)0 =1

            Hence, Kp = Kc

So, for all reactions with dn = 0, Kp = Kc.

Correct option= B, E


Related Solutions

A.) For which reaction will Kp = Kc? 2 H2O(l) ↔ 2 H2(g) + O2(g) 2...
A.) For which reaction will Kp = Kc? 2 H2O(l) ↔ 2 H2(g) + O2(g) 2 HgO(s) ↔ Hg(l) + O2(g) S(s) + O2(g) ↔ SO2(g) H2CO3(s) ↔ H2O(l) + CO2(g) CaCO3(s) ↔ CaO(s) + CO2(g) B.) How does an increase in the pressure within the container by the addition of the inert gas E affect the amount of C present at equilibrium for the following reaction? A(g) + 3 B(g) ↔ 2 C(g) + D(g)           ΔH° = -65 kJ...
Part A Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) Express your answer using...
Part A Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) Express your answer using three significant figures. Kc=? Part B Calculate Kc for the reaction below. CH4(g)+H2O(g)⇌CO(g)+3H2(g)Kp=7.7×1024 (at 298 K) Express your answer using two significant figures. Kc=
At 22°C, Kp = 0.070 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) a)...
At 22°C, Kp = 0.070 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) a) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains. b) After the equilibrium in part a) was established, the reaction flask is then charged with an additional 0.59 atm of NH3. When the system has equilibrated, what is the partial pressure of hydrogen sulfide?
For which of the following reactions is Δ H ∘ rxn equal to Δ H ∘...
For which of the following reactions is Δ H ∘ rxn equal to Δ H ∘ f of the product(s)? You do not need to look up any values to answer this question. Check all that apply. Check all that apply. BaC O 3 (s)→BaO(s)+C O 2 (g) C(s,graphite)+ O 2 (g)→C O 2 (g) CO(g)+ 1 2 O 2 (g)→C O 2 (g) 2Na(s)+ F 2 (g)→2NaF(s) Na(s)+ 1 2 F 2 (l)→NaF(s) Na(s)+ 1 2 F 2 (g)→NaF(s)...
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =...
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP = 0.032 at a particular temperature. At that temperature, a vessel is filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm of NO (g). What is the pressure of NO (g) at equilibrium?
In which direction will the net reaction proceed.X(g) + Y(g) <==> Z(g) .. Kp = 1.00...
In which direction will the net reaction proceed.X(g) + Y(g) <==> Z(g) .. Kp = 1.00 at 300kfor each of these sets of initial conditions? 1) [X] = [Y] = [Z] = 1.0 Ma] net reaction goes to the left [this one?]b] net reaction goes to the rightc] reaction is at equilibrium2. Px = Pz = 1.0 atm, Py = 0.50 atm a] net reaction goes to the leftb] net reaction goes to the rightc] reaction is at equilibrium
Which of the following reactions is spontaneous as written? C(s) + 2H2 (g) = CH4 (g)...
Which of the following reactions is spontaneous as written? C(s) + 2H2 (g) = CH4 (g)            2H2 (g) + O2 (g) = 2H2O(l)       4HCN(g) + 5O2(g) = 2H2O(l) + 4CO2(g) 2N2(g) NaI(s) = Na+(aq) + I-(aq)
Ammonia reacts with oxygen to form nitrous monoxide and water as in the following equation: 4NH3(g)...
Ammonia reacts with oxygen to form nitrous monoxide and water as in the following equation: 4NH3(g) +5O2=4NO(g) + 6H2O(g) How many liters of H2O gas can be produced given a temperature of 48° c and a pressure of 975 torr from 145.0 grams of NH3?
Given the equation: PCl3(g) + Cl2(g) ⇌ PCl5(g) kp = 1.05 at 70.5 °C If one...
Given the equation: PCl3(g) + Cl2(g) ⇌ PCl5(g) kp = 1.05 at 70.5 °C If one starts with 1,7 atm of PCl5(g), what is the partial pressure of PCl5(g) at equilibrium?
Find the temperature in ºC at which Kp = 43.7 for the reaction H2(g) + I2(g)...
Find the temperature in ºC at which Kp = 43.7 for the reaction H2(g) + I2(g) ⇌ 2 HI(g). Use ∆Hºrxn and ∆Sºrxn to calculate and assume that they are independent of temperature. Use the thermodynamic data in the appendix of your textbook; I have provided the needed appendix on BlackBoard for your convenience. Report your answer to zero places past the decimal.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT