Chemistry Answers

Which term of the sequence 3, 12, 48,... is equal to 196 608?

Is it 12th, or, 10th, or 11th, or 9th.

how many grams of O2 will react completely with 35.0 grams of PH3?

Calculate the percentage of hydrogen (by mass) in C5H8.

1) At a particular temperature k= 6.7x10^-6 for the following reaction:

2Br2(g) +O2(g) -> 2Br2O(g)

In an experiment in which 1.0 mol of Br2 and 1.0 mol of O2 are mixed in a 2.5-L vessel, what are the equilibrium concentrations of all gases?

2) At a particular temperature k= 6.5x10^-6 for the following reaction:

2Cl2(g)+O2(g) -> 2Cl2O(g)

In an experiment in which 2.0 mol of Cl2 and 1.5 mol of O2 are mixed in a 2.0-L vessel, what are the equilibrium concentrations of all gases?

The equilibrium constant, K_p, for the following reaction is 2.01 at 500 K:

PCl₃(g) + Cl₂(g) PCl₅(g)

Calculate the equilibrium partial pressures of all species when PCl₃ and Cl₂, each at an intitial partial pressure of 1.47 atm, are introduced into an evacuated vessel at 500 K.

Define Le Chatelier’s Principle

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

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

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

Q9: Calculate the standard free energy change for the combustion of methane at 250^oC. Again, assume that all reactants and products are gases. 3 SIG FIGURES.

Q10 PART A: Calculate the free energy change for the combustion of methane at 250^oC. Assume that all reactants and products are gases and that the partial pressures of the various gases of interest are: methane = 0.56 atm, oxygen = 0.45 atm, carbon dioxide = 2.10 atm, water = 3.40 atm.

PART B: What is the value of the equilibrium constant for the reaction described in Question 10? Provide an answer correct to 2 significant figures.

PART C: Based on your calculations in previous problems, at what temperature will the combustion of methane be at equilibrium? Provide an answer correct to 2 significant figures