1. For the reaction ICl(g) %g) C(g), K-22x 10 at 25°C. Calculate K, at this temp
ID: 715038 • Letter: 1
Question
1. For the reaction ICl(g) %g) C(g), K-22x 10 at 25°C. Calculate K, at this temperature for lag) + Cl2(g) iCl@ 2. For the reaction SO Clh(g) SO(g) Clh(g), K -0.011 at a particular temperature. A 2.00 L container at this temperature contains 0.30 mole SO2, 0.20 mole Clh, and 0.50 mole SO2Cl2. a) Is this system at equilibrium? b) If it is not at equilibrium, in which direction will the system move to reach equilibrium? Why 3. For the reaction SO-(8)+NO-(g) NO(g) + so,(g), K-85.0 at 4.60 x 102 °C. A reaction is started with 0.0500 M of both reactants (Note, initially no products). a) Calculate the equilibrium concentration in M of all species. (If you correctly set-up the ICE chart for this problem, you will see the equilibrium constant expression is a perfect square & so the quadratic formula is not needed. If yours is not a perfect square, check your work.) b) Calculate the equilibrium partial pressures in atm of all species. 4. Oxygen dissociates into gaseous atoms according to the equilibrium 0° 20 g). At 1800 K the equilibrium constant K.-1.2x 1010. One (1.00) mole of O2 is placed in a 5.0 L flask, heated to 1800 K, and allowed to come to equilibrium at this temperature. Find the equilibrium concentration of all species at 1800 K. (Make a simplifying approximation and check it.) 5. For the system CO2(g) + H2(g) CO(g) + H2O(g), K.-0640 at a certain temperature. Calculate the equilibrium concentrations of all species in M if the reaction is started with 1.00 M CO2, 1.00 M H2 and 1.00 M Co. (Note, initially H20 is not present)Explanation / Answer
1)
ICl ---> 1/2 I2 + 1/2 Cl2
Kc = [I2]^(1/2)* [Cl2]^(1/2) / [ICl]
Kc = ([I2]*[Cl2] )^(1/2) / [ICl]
take square on both side
Kc^2 = [I2]*[Cl2] / [ICl]^2
[ICl]^2 / [I2] * [Cl2] = 1 / Kc
I2 +Cl2 ---> 2 ICl
Kc' = [ICl]^2 / [I2] *[Cl2]
Kc' = 1/Kc^2
= 1 / (2.2*10^-3)^2 = 1 / 4.84 *10^-6
Kc' = 0.2066*10^6
Kc' = 2.066*10^5
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