Reactions
Determine the products for this reaction:
C3H8 + O2 --->?
What are CO2 and H2O because it is a combustion reaction?
What is the overall reaction order for the following?
Rate = k[A][B]2/[C]
What is second?
This is the conjugate base of HCO3-.
What is CO32-?
If a reaction has a Keq = 4.0 x 10-6, which side of the reaction is favored at equilibrium? Why?
What is the reactants/left side are favored because K<<1?
If Q>K, which direction does the reaction shift to reach equilibrium?
What is to the left/towards the reactants?
A student dissolves 11.7 g NaCl in enough water to make 250.0 mL of solution. Determine the molarity.
What is 0.801 M?
For the elementary reaction, write the predicted rate law.
NO + Cl2 --> NOCl
What is Rate = k[NO]2[Cl2] ?
Based on this equilibrium constant (Ka = 1.0 x 10-7), comment on the relative strength of this acid (with evidence).
What is it is a weak acid because its equilibrium constant << 1?
If [H+] = 1.0 x 10-9, is the solution acidic or basic (no math)? How do you know?
What is the solution is basic because the concentration of protons is smaller than 1.0 x 10-7?
Write the equilibrium expression for:
N2 (g) + H2 (g) --- NH3 (g)
What is Kc= [NH3]2/[N2][H2]3?
When aqueous barium nitrate reacts with sodium sulfate, this precipitate forms.
What is BaSO4 (s) ?
For a second-order reaction, these are the units of the rate constant.
What is 1/Ms?
One acid has a Ka = 1.0 x 10-3, while another has a Ka = 1.0 x 10-8. This acid has the stronger conjugate base.
What is the acid with Ka = 1.0 x 10-8?
For the following reaction, predict the shift when you decrease the volume of the reaction.
2NO (g) + O2 (g) -- 2NO2 (g)
What is it is going to shift to the right/products?
For an exothermic reaction at equilibrium, predict the effect of increasing temperature.
What is the equilibrium shift left/towards the reactants?
In the following reaction, identify the limiting reagent if you react 10.0 g Al with 10.0 g of Cl2?
2Al + 3Cl2 --> 2AlCl3
What is Cl2?
NH3 (g) + O2 (g) → NO (g) + H2O (g)
At a certain moment, the concentration of O2 is decreasing at a rate of:
Δ[O2]/Δt = -0.125 M/s
Calculate the rate of formation of NO.
What is 0.100 M/s?
A weak acid has a Ka = 4.0 x 10-6. What is the Kb of its conjugate base?
What is Kb = 2.5 x 10-9?
A student titrates 25.0 mL of an unknown HCl solution with 0.200 M NaOH. The equivalence point is reached after 31.50 mL of NaOH is added. What was the original concentration of the HCl solution?
What is 0.252 M HCl?
Fe3O4 (s) + H2 (g) ⇄ Fe (s) + H2O (g)
At a certain temperature, Kc = 0.50. A mixture is prepared with [H2] = 0.10 M and [H2O] = 0.50 M. Calculate Qc and comment on the shift of the reaction.
What is the reaction quotient is 625, meaning the reaction will shift to the left?
How much excess reactant (moles) is left over when 50 mL of .250 M iron (III) chloride (FeCl3) is reacted with 50 mL of .250 M sodium carbonate (Na2CO3) solution?
What is 0.0041 moles of FeCl3 left over?
Based on the proposed mechanism, write the overall rate law:
(1) 2A = B + D (fast, eq)
(2) B + D --> E + C (slow)
(3) E --> 2 B (fast)
What is Rate = k[A]2?
Calculate the pH of 0.20 M HF if the Ka = 6.8 x 10-4.
What is pH = 1.92?
RANDOM DOUBLE JEOPARDY: Where was the caesar salad invented?
Where is Mexico?
Calculate the equilibrium concentrations of all species (H2, I2, HI) if the reactants' initial concentrations are [H2] = 1.000 M and [I2] = 2.000 M. The Kc = 50.5.
What is H2 is 0.065 M, I2 is 1.065 M, and HI is 1.87 M?