reactions and equilibrium constants are hypothetical, chemistry homework help

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**** All reactions and equilibrium constants are hypothetical. The enthalpies of reaction are also hypothetical. They are used for your practice and should not be taken as true values.

1: Explain with reason why or why not the following reactions are at equilibrium.

A bottle of glue is opened and spread on a piece of paper.

2: Explain with reason whether the following reactions would have a high K, a low K, or a K around 1.

In the ocean, chloride ions join together to make chlorine gas, which is poisonous.

3: The following reactions are at equilibrium. The enthalpy is given. How will the reactions shift with the changes listed after.

HCO3-(aq) + H+(aq)H2CO3(aq), ΔH = -10kJ/mol. 1) sodium bicarbonate is inserted into the container. 2) carbonic acid is removed. 3) Argon is added to the container. 4) The temperature is raised. 5) Sodium hydroxide is added to the container.

4: Look at the following reactions. The initial conditions are stated. Using the reaction quotient, determine which way the reaction will shift. All conditions are given in mol dm-3 unless otherwise stated.

Pb+2(aq) + 2OH-(aq)Pb(OH)2(s), Kc= 7×10^19, [Pb2+] = 1.4 x 10^-5, [OH-] = 1.2 x 10^-6, Pb(OH)2 = 1gram in one liter.

5: Look at the following equilibrium constants for the following reactions.

H2(g) + F2(g)2HF(g), Kc = 1.4 x 10^9

H2(g) + Cl2(g)2HCl(g), Kc = 1.4 x10^7
H2(g) + I2(g)2HI(g), Kc = 1.4x 10^5
3H2(g) + CO(g)CH4(g) + H2O(l), Kc=1.3×10^-4
What is the equilibrium constant for the following reactions?

HF(g) + 0.5Cl2(g)HCl(g) + 0.5F2(g)

6. Using the initial conditions, determine the equilibrium conditions. All conditions are given in mol dm-3 unless otherwise stated.

Pb(OH)2(s)Cu+2 (aq) + 2OH—(aq) , Kc= 1.4 x 10-20, [Pb2+] = 5.1 x 10-6, [OH-] = 3.4 x 10-5, Pb(OH)2 = 1gram in one liter.

7.Using the initial conditions, determine the equilibrium conditions. All conditions are given in mol dm-3 unless otherwise stated.

H2(g) + I2(g)2HI(g), Kc = 1.4 x 105, [H2] = 0.1, [I2] = 0.01, [HI] = 0.5

8. Using the initial conditions, determine the equilibrium conditions. All conditions are given in mol dm-3 unless otherwise stated.

CO2(g) + CaO(s)  CaCO3(s), Kc = 1.2 x 10-8, [CO2] = 3 x 10-4. Inside the one liter container, there is 40 grams of calcium oxide and 10 grams of calcium carbonate.

9. Change the following Gibbs Energies into Kc. Assume the temperature is at room temperature. A) 112kJ/mol
B) 12 kJ/mol
C) -10kJ/mol

D) 54 kJ/mol

10: Find the rate constant of the reverse reaction for the following.

Kc = 8 x 102. The rate constant of the forward reaction is 10.

 
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