Each of the containers shown is at the same temperature, and contains the same number of molecules. In which container is the gas densest?
At 200.0 K, a gas fills a 475.0 mL balloon. What will be the volume of the balloon if the temperature is raised by 60.0 K?
Once a system has reached equilibrium, what happens to:
a) The rates of the forward and backward reactions
b) The concentration of the species present
Methanol is a very important starting material in the chemical industry. A key reaction in its
manufacture is:
CO(g) + 2H2(g) ⇌ CH3OH(g) + 52 kJ
a) Write an expression for the equilibrium constant K
i) In an equilibrium mixture at 100°C the following gas concentrations were found:
CO : 3.76 x 10-3 mol L-1 H2: 4.30 x 10-3 mol L-1
CH3OH: 4.17 x 10-10 mol L-1
Calculate the value of K(eq) at 100°C
ii) Calculate the concentration of methanol produced by the reaction in (b), with the
following reactant concentrations:
CO: 2.13 x 10-3 mol L-1
H2: 1.4 x 10-3 mol L-1
b) Define Le Chatelier’s Principle
c) Explain the effect on the equilibrium concentration of methanol if the temperature
is raised
d) A safety valve in the reaction vessel is temporarily opened to release the high
pressure gasses. Describe the effect it has on the equilibrium position and the
equilibrium constant K
Consider the exothermic reaction: A + B ⇌ C + Heat
Compare the activation energy for this reaction in the forward and reverse
directions.
Draw an energy profile diagram to illustrate your answer
what is the time required to pass 1 F of electricity through electrolyte with a current of 0.35 ampere
• what is the mass in grams of 1.204 x 10²³ molecules of H2O?
• how many formula units are there in 0.175 g of LiF
How many moles of water are equal to 1.204 x 10²³ molecules of H2O?
provide a solution.
What is the mass percentage of O in C₃H₈O₂?
When an electron is added to the valence shell