Potassium Thiocyanate in aqueous solution, At 23.89 degree C,
rate law constant 0.437M^-2min^-1. Lab mates found...
Potassium Thiocyanate in aqueous solution, At 23.89 degree C,
rate law constant 0.437M^-2min^-1. Lab mates found that at 15.55deg
C the rate law constant was 0.0507M^-2min^-1 R=8.314 J/mol*K What
is the activation energy for this?
When an aqueous solution of strontium chloride is added to an
aqueous solution of potassium sulfate, a precipitation reaction
occurs. Write the balanced net ionic equation of the reaction.
1. An aqueous solution of potassium hydroxide is standardized by
titration with a 0.117 M solution of hydrobromic acid. If 18.7 mL
of base are required to neutralize 15.7 mL of the acid, what is the
molarity of the potassium hydroxide solution?
2. .An aqueous solution of nitric acid is standardized by
titration with a 0.183 M solution of calcium hydroxide. If 28.5 mL
of base are required to neutralize 21.4 mL of the acid, what is the
molarity of...
If a 1st order reaction has a rate constant of 2.30 s^-1 at 25
degree C, and at a frequency factor of 2.51*10^5, calculate the
activation energy.
A) 9715 J/mol
B)186 J/mol
C) -186 J/mol
D) 2.51*10^4 J/mol
E) 2.51*10^-4 J/mol
1) What is the pH of a 0.187 M aqueous solution of potassium
fluoride, KF?
2) What is the pH of a 7.42×10-2 M aqueous solution of ammonium
nitrate, NH4NO3 ?
Please show work, I'm confused on how to solve when NO Ka or Kb
value is given in the problem!
The mole fraction of potassium phosphate, K3PO4, in an aqueous solution is 8.11x10-2 The percent by mass of potassium phosphate in the solution is _______ %. The mole fraction of ammonium sulfide, (NH4)2S, in an aqueous solution is 3.42x10-2 The percent by mass of ammonium sulfide in the solution is _______ %.
A.What concentration of potassium hydroxide is
needed to give an aqueous solution with a pOH of
3.720?
Molarity of potassium hydroxide =
B.What concentration of sodium hydroxide is
needed to give an aqueous solution with a pH of
9.210?
Molarity of sodium hydroxide =
An aqueous solution of glycerin, 7% by weight, is prepared. The
solution is found to have a density of 1.0149 g/mL. The density of
pure glycerin (MW=92.0473) is 1.2609 g/mL. What is the molarity and
molality concentration of the solution?
The iodine clock reaction involves reacting an aqueous solution
of potassium iodate with another solution containing sulfuric acid,
sodium bisulfite, and starch. The reaction begins colourless but at
a certain point the free triiodide concentration builds up,
complexing with the starch molecules and producing a dark blue to
almost black colour almost instantaneously. Which of the following
options will cause the blue colour to appear faster?
Increasing pH
Increasing bisulfite concentration
Increasing starch concentration
Decreasing temperature
Increasing temperature
1. The rate law for a given reaction is rate = k[NOBr]2. The
rate constant is 1.0 x 10-5 1/M∙s, and the initial concentration
was 0.100 M. What is the first half-life of this reaction?
A) 0.50 s B) 6.9 x 104 s C) 1.0 x 10-5 s D) 1.0 x 106 s E) None
of these
2. The reaction SO2Cl2 SO2 + Cl2 is first order in SO2Cl2. If
the concentration of SO2Cl2 after 198 s is 1.47 x...