1)A reaction(A-products) is found to be first order with a rate constant of 2.97*10^-3 / min. What is the half life for this reaction?

2) If the reaction described in probrem 1 starts with an initial concentration of 1.00M of reactant A, What is the concentration of A after 300min?

3) What is the reaction oreder and what is the value of the rate constant?

IN(H2O2) y=0.00835x-0.00493

1/H2O2 y=0.00460x-0.847

H2O2 y=-0.000264x+0.841

Estimate the boiling point of benzene given that its vapour pressure is 20 kPa at 35C and 50.0 kPa at 58.8C. Please show work.

your percent yield of Cu(NH3)4SO4*H20is dependent on the quality of your laboratory technique. give three examples of errors in technique that would lower the percent yeild of the sythesis briefly explain how each error would lower the percent yeild

Distinguish between all the inter-molecular forces and give an example of each. (Please explain as if you'd teach a child....i'm very poor with this).

You are titrating 25.00 mL of a 0.100 M solution of a weak acid with a 0.250 M solution of potassium hydroxide. Assume the pKa of the weak acid is 5.6.

A. What is the pH after adding 3.0 mL of 0.250 M potassium hydroxide?

B. What is the pH at the midpoint of the titration?

C. What is the pH at the equivalence point of the titration?

Problem #C4:

A) Calculate the Molarity for: H⁺(at equilibrium) and HCl (after dilution occurs but before the reaction occurs).

B) Calculate the Molarity for: H⁺(at equilibrium) and NaOH (after dilution occurs but before the reaction occurs).

C. pH of Buffer Solutions:

1. Preparation of Buffer Solution: Weigh 3.3 g of solid sodium acetate trihydrate, NaC2H3O2 * H2O, into a clean 150 or 250 mL beaker. Using graduated cylinders, add 46 mL of deionized water and 4.0 mL of 6.0 M HC2H3O2. Mix thoroughly. Measure 19.0 mL of this into each of two clean beakers. Label as "A" and "B". Measure the pH of this buffer solution using the remaining 10 mL.

2. Addition of Acid or Base to Buffer: a. To the buffer in beaker "A", add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture. b. To the buffer in beaker "B,", add 1.0 mL of

3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture. 3. pH of Deionized water: Obtain 19 mL of deionized water in each of two beakers. Read the pH of the deionized water. (NOTE: It will not be a pH of 7.00.)

4. Addition of Acid or Base to Deionized Water: a. To one beaker of deionized water, add 1.0 mL of 3.0 M HCl. Mix thoroughly and read the pH of the resulting mixture. b. To the second beaker of deionized water, add 1.0 mL of 3.0 M NAOH. Mix thoroughly and read the pH of the resulting mixture.

Aldehydes with strongly electron donating groups, such as p-dimethylaminobenzaldehyde, or with strongly electron withdrawing groups, such as p-nitrobenzaldehyde, fail to undergo self-condensation in the presence of cyanide ion. However such aldehydes will undergo mixed condensations with benzaldehyde. Explain.

Why might a reaction with a very negative gibbs free energy not happen, such as hydrogen reacting with oxygen? And what is the concentration of a reactant after 3 half-lives, if the reaction in the question is first order

Two 25.0 ml samples, one 0.100 mol/L HCl and the other 0.100mol/L HF, were titrated with 0.200 mol/L KOH.

a)What is the volume of added base at the equivalence point for each titration?

b)Predict whether the pH at the equivalence point for each titration will be acidic, basic or neutral? Explain your selection.c)Predict which titration curve will have the lower initial pH and explain your selection.

A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: 2NO(g)+2H2(g)←−→N2(g)+2H2O(g) At equilibrium [NO]=0.062M. Calculate the equilibrium concentration of H2. Calculate the equilibrium concentration of N2. Calculate the equilibrium concentration of H2O. Calculate Kc

A solution is made by mixing 13.0 g of Sr(OH)2 and 50.0 mL of 0.150 M HNO3.

A.Write a balanced equation for the reaction that occurs between the solutes.

B.Calculate the concentration of OH− ion remaining in solution.

C.Calculate the concentration of Sr2+ ion remaining in solution.

D.Calculate the concentration of NO−3 ion remaining in solution.

E.Is the resultant solution acidic or basic?

3 SHOW ALL WORK STEP BY STEP WITHOUT SHORT CUTS

1) make a solution of 0.25% n-propanol (use 25 ml volumetric flask)

2) make a water solution of methanol and isopropanol of 0.2% make it in the same container and in separated container.

3) make a 50ml stock solution of 0.50 wt% ethanol .

4) make five solution ranging from of ethanol 0.0 %, 0.05%, 0.10%, 0.20,% 0.30% 0.40% 0.50% wt% in water. (Used 25ml volumetric flasks)

Which of the following statements about insulin is INCORRECT?

1.

a. Using Beer-Lambert equation (A=eCL) to explain how absorbance is affected by changes in concentration and in the pathlength.

b. How to use the molecular structure to predict which molecules will absorb radiation in the IR region

c. Explain the mechanism by which greenhouse gases result in higher atmospheric temperature.

d. Explain why the wavelength at which a molecule absorbs energy is important in determining whether a molecule will act as a greenhouse gas.

e. Explain the importance of the solar window and the atmospheric window (also called thermal window)