1 mL of a 5.0 nM enzyme solution is rapidly mixed into 9 mL of a...

1 mL of a 5.0 nM enzyme solution is rapidly mixed into 9 mL of a 0.50 µM substrate solution, and the rate of formation of product is found to be 0.490 µM/s.

a) What are the initial concentrations of enzyme and substrate in the 10 mL mixture?

b) Calculate the Michaelis constant of the complex (KM), knowing that the rate of formation of product saturates to 0.670 µM/s when the experiment is performed with a highly concentrated substrate solution instead of the 0.50 µM substrate solution

Expert Solution

Amanda K answered 6 months ago

5.0 g of calcium phosphate is mixed into 1 L of solution a) what is the...

5.0 g of calcium phosphate is mixed into 1 L of solution a) what is the concentration of Ca^2+ and PO4^3-? calculate b) explain how you could dissolve will calcium phosphate c) what is the molarity of the solutions, if you were able to dissolve all of it?

35.40 mL of a 1.20 M solution of KCl is mixed with 55.0 ML of a...

35.40 mL of a 1.20 M solution of KCl is mixed with 55.0 ML of a solution of Pb(NO3)2 with unknown Molarity. 2KCl(aq) + Pb(NO3)2(aq) -->2KNO3(aq) + PbCl2(s). The solid PbCl2 weights 5.29g. If the concerntration of lead (II) ions in solution after the complete precipitation is 0.3564 M, what was the original concentration of the lead(II) nitrate solution

50 mL of 0.010 mol.L-1 Na2SO4 solution was mixed with 50 mL of 0.20 mol.L-1 KNO3...

50 mL of 0.010 mol.L-1 Na2SO4 solution was mixed with 50 mL of 0.20 mol.L-1 KNO3 solution, calculate the ionic strength of the mixed solution. I need to complete solution, please

A solution of 100 mL of .200M sodium chromate is mixed with a solution of 200...

A solution of 100 mL of .200M sodium chromate is mixed with a solution of 200 mL of 0.150M strontium nitrate. What is the is the limiting reagent or reacting? How many grams of percipitate forms? What is the concentration of spectator ions in the final mixture? What is the concentration of the excess ion?

A 160.0 mL solution of 2.813 M strontium nitrate is mixed with 215.0 mL of a...

A 160.0 mL solution of 2.813 M strontium nitrate is mixed with 215.0 mL of a 2.900 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. Mass = 39.2 g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a zero for the concentration. [Na+] = ? [Sr2+]=0.37 M [F-]= 0 M [NO3-]= ?

A 200 mL solution of 0.100 M solution of Ammonia, NH3 , is slowly mixed with...

A 200 mL solution of 0.100 M solution of Ammonia, NH3 , is slowly mixed with 0.100 M HCl. Determine the pH after addition of: 0 mL of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, 250 mL of HCl 4. Describe in exact detail (including gram quantities and identity of species) how you would create a 500 mL solution of buffer with a pH 8.0 ?

375 mL of a .150 M aqueous solution of silver (1) nitrate is mixed with 125...

375 mL of a .150 M aqueous solution of silver (1) nitrate is mixed with 125 mL of .125 M aqueous solution of sodium phosphate. Calculate the mass of precipitate that forms and the final concentration of each ion in the mixed solution. Volumes are additive and the precipitation reaction goes to completion.

Ancef, an antibiotic, is mixed as 50 mL of IV solution. It is to infuse in...

Ancef, an antibiotic, is mixed as 50 mL of IV solution. It is to infuse in 1 hour. The drop factor of the infusion set is 60 gtt/mL. What is the flow rate?

A 130.0 mL sample of a solution that is 0.0126 M in NiCl2 is mixed with...

A 130.0 mL sample of a solution that is 0.0126 M in NiCl2 is mixed with a 190.0 mL sample of a solution that is 0.400 M in NH3. -After the solution reaches equilibrium, what concentration of Ni2+(aq) remains? The value of Kf for Ni(NH3)62+ is 2.0×108.

If 15.0 mL of a 1.5M HCl solution at 21.50C is mixed with 25.0mL of a...

If 15.0 mL of a 1.5M HCl solution at 21.50C is mixed with 25.0mL of a 1.5M NaOH solution at 21.50C that is in a calorimeter, and the final mixed solution temperature rises to28.50C, what is the ΔHrxnfor this process?Assume that Ccalorimeter= 35.5J/0C. a.What is the balanced equation for the reaction? b.What is the source of the heat that is causing the increase in temperature? c.Calculate the amount of heat absorbed or lost for the HCl/NaOH solution. Assume aqueous conditions.(Cwater=...

Question