chem help ?

I’m working on a Chemistry exercise and need support.

  • Write the equilibrium constant expression for the following balanced reactions.
  • a. 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

    b. NH3(g) + HCl(g) ⇌ NH4Cl(s)

    c. 2 NO2(g) ⇌ N2O4(g)g

    d. Ni2+(aq) + 6 NH3(aq) ⇌ Ni(NH3)62+(aq)

    e. HF (aq) + H2O(l) ⇌ H3O+ (aq) + F (aq)

  • For the general reaction A + B ⇌ C + D, and given the value of K, state whether the equilibrium favors the reactants, products or neither.
    • K = 3.75 x 1015
    • K = 1.44 x 10-5
    • K = 24
    • K = 0.0199
  • For the reaction CO(g) + 2 H2(g) ⇌ CH3OH(g), the equilibrium concentrations are 0.495 M carbon monoxide gas, 0.990 M hydrogen gas and 0.00533 M methanol gas.What is the equilibrium constant for this reaction?
  • Name two ways to shift the reaction below to products (right side).
  • Consider the system at equilibrium:
  • 2 SO2(g) + O2(g) ⇌ 2 SO3(g)
  • NH3(g) + HCl(g) ⇌ NH4Cl(s)
  • 2 NO2(g) ⇌ N2O4(g)g
  • Ni2+(aq) + 6 NH3(aq) ⇌ Ni(NH3)62+(aq)
  • HF (aq)+H2O(l) ⇌ H3O+ (aq)+ F (aq)

H2(g) + Br2(g)⇌ 2 HBr (g) + heat

2 SO3(g) +197.8 kJ 2 SO2(g)+ 1 O2(g)

Predict how the equilibrium will shift (towards reactants/left or towards products/right) if:

  • oxygen gas is added
  • SO2(g) is removed from the system
  • the temperature is decreased
  • SO3(g) is added
  • Increase in pressure
  • a catalyst is added to the system

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