the following data were acquired in an experiment like ours where the initial amount of hydrogen peroxide is 0.0035 moles. Find the rate constant.

0.0000753 0.008 0.0003466 1.839 0.0007398 4.150 0.0010596 7.423

A solution contains Al3+ and Co2+. The addition of 0.3628 L of 1.714 M NaOH results in the complete precipitation of the ions as Al(OH)3and Co(OH)2. The total mass of the precipitate is 21.96 g. Find the masses of Al3+and Co2+ in the solution.

A 10.0 g piece of pure aluminum is placed in 75.0 mL of 0.54 M hydrochloric acid at STP condition. They react as follows: 2Al + 6HCl → 3H2(g) + 2AlCl3 Calculate the following:

a. Volume, in liters, of hydrogen gas.

b. Molarity of Al+3. (Assume 75.0 mL solution.)

c. Molarity of Cl–. (Assume 75.0 mL solution.)

For each reaction, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base-

HBr(aq)+H2O(l)→H3O+(aq)+Br−(aq) Express your answers as a chemical expressions. Enter your answers in order given in the question separated by commas. NH3(aq)+H2O(l)⇌NH+4(aq)+OH−(aq) Express your answers as a chemical expressions. Enter your answers in order given in the question separated by commas. HNO3(aq)+H2O(l)→H3O+(aq)+NO−3(aq) Express your answers as a chemical expressions. Enter your answers in order given in the question separated by commas. C5H5N(aq)+H2O(l)⇌C5H5NH+(aq)+OH−(aq) Express your answers as a chemical expressions. Enter your answers in order given in the question separated by commas.

1.)

What is the rate law for the following mechanism in terms of the overall rate constant kkk?

A-

Express your answer in terms of kkk and the necessary concentrations (e.g., k*[A]^3*[D]).

B-

Consider the reaction

2X2Y2+Z2⇌2X2Y2Z2X2Y2+Z2⇌2X2Y2Z

which has a rate law of

rate=rate= k[X2Y2][Z2]k[X2Y2][Z2]

Select a possible mechanism for the reaction.

View Available Hint(s)

Consider the reaction

which has a rate law of

Select a possible mechanism for the reaction.

When did you finally stoped heating Cu and sulfur mixture in chemical reaction of copper lab? Which of the following are redox reactions ?

Explain your answer on the basis of changes in oxidation number. 1. CuSO4 + 2NaOH → Cu(OH) 2 + Na 2SO4

2. 2Al + 3MgSO4 → 3Mg + Al 2(SO4)3

3. 2(NH4)3PO4 + 3Ba(NO3)2 → Ba 3(PO4)2 + 6NH4NO3

4. 2HNO3 + 3H3AsO3 → 2NO + 3H 3AsO4 + H2O

For the following reaction, 22.0 grams of iron are allowed to react with 45.3 grams of chlorine gas . iron(s) + chlorine(g) iron(III) chloride(s) . What is the maximum mass of iron(III) chloride that can be formed? ____grams . What is the FORMULA for the limiting reagent?. What mass of the excess reagent remains after the reaction is complete?____ grams

ORGANIC CHEMISTRY:

Draw a balanced chemical reaction for the synthesis of methyl salicylate from aspirin tablets. Calculate the theorectical yield for the product in grams using the limiting reagent aspirin, remembering you are extracting FOUR aspirin tablets and there is 325 mg of aspirin in each one.

Calculate DG for the following reaction if the partial pressure of CO₂ is .05 atm at 25^oC.

CaCO₃(s) yields CaO(s) + CO₂(g)

--------------------------------------------------------

Ca(s) + CO₂(g) + 1/2O₂(g) yields CaCO₃(s)             DH^o=-814.1kJ                        DS^o=-266.3J

2Ca(s) + O₂(g) yields 2CaO(s)               DH^o=-634.9kJ                        DS^o=-250.3J

In a laboratory experiment, 50.0 g of gaseous propane (C3H8) was heated in the presence of air (O2) to produce gaseous carbon dioxide and gaseous water. upon completion of the experiment, 13.0 g of carbon dioxide were obtained.

Balanced Equation: C3H8 (g) + 5O2 (g) --> 3CO2 (g) + 4H2O (g)

a) What is the limiting reactant?

b) what is the theoretical yield?

c) what is the percent yield?

For Ammonia synthesis reaction: 3H2(g)+N2(g)?2NH3, Under 673 K, 1000 kPa, the initial molar ratio of H2 and N2 is 3:1 and then this reaction reach equilibrium. The molar ratio of NH3 is 0.0385. Calculate (1) the standard equilibrium constant under this condition. (2) At 673 K, the total pressure of this system if the molar ratio of NH3 is 0.05.

Spectrophotometric Analysis of Fe2+ using 1,10-phenanthroline

Given the following data, calculate the percent by mass Fe²⁺ in the unknown sample. Assume the experimental data provided is obtained using the same procedure you will be using in the lab.

Unknown sample mass = 0.1725

Absorbance (average) of unknown sample = 0.374

Beer’s Law Data:        Slope = 0.2203 L/mg Fe²⁺

                                    y-intercept = -0.001

**PREPARATION OF UNKNOWN FE2+ SAMPLE**

weighed 0.1725 g of the unknown sample into 100 mL beaker -> add about 30 mL of distilled water and 1 mL concentrated sulfuric acid -> transferred to 100 mL volumetric flask, then filled to mark with distilled water -> pipet 10.00 mL into second 100 mL volumetric flask and make up to the mark -> then pipette 10.00 mL into third 100 mL volumetric flask and add 10 mL saturated sodium acetate and 10 mL 10% hydroxylamine hydrochloride -> add 10 mL 0.1% 1,10-phenanthroline to the flask then fill to mark with distilled water

Which of the following statements are incorrect?

a) The main source of NOx in the stratosphere is the reaction of O(1D) with N2O

b) Some ClOx in the stratosphere is produced by photolysis of CH3Cl which originates from the oceans.

c) Some stratospheric NOx is produced by oxidation of N2 by lightning.

d) The main source of ClOx in the stratosphere is photolysis of CFCs.

e) The main source of HOx in the stratosphere is photolysis of H2O.

An analytical chemist decides to analyze a given sample spectrophotometrically for its copper content.  The chemist knows that copper(I) ions form a colored coordination complex with neocuproine (ncup), C₁₄H₁₂N₂, in a one-to-two ratio, Cu(ncup)₂⁺.  The chemist also knows that Cu(ncup)₂⁺ is more soluble in 3-methyl-1-butanol than in water and that Cu(ncup)₂⁺ in 3-methyl-1-butanol shows an absorbance maximum at 454 nm.  Thus, the chemist proceeds with the chemical analysis.  She treats 0.1482 g of copper wire, 98.50% (w/w) pure, with a minimum volume of concentrated nitric acid in order to get all of the copper metal into solution (aqueous) as copper (II) ions.  After neutralizing the copper-containing solution with base, the chemist transfers the solution quantitatively to a 500.0-mL volumetric flask and then dilutes the solution with deionized water up to the mark on the flask.  Next, the chemist treats 10.00 mL of the solution with a reducing agent in order to convert copper(II) ions to copper(I) ions and then adds a buffer in order to change the pH of the solution to one for which complexation between copper(I) ions and neocuproine occurs readily.  Subsequently, the chemist treats the resulting solution with neocuproine to complex all of the copper(I) ions and then adds 100.00 mL of 3-methyl-1-butanol.  After shaking well to make sure that essentially all of the Cu(ncup)₂⁺ is extracted by the 3-methyl-1-butanol from the aqueous solution, the chemist separates the aqueous layer (bottom) completely from the 3-methyl-1-butanol layer (top) and then quantitatively transfers the 3-methyl-1-butanol layer to a 1.000-L volumetric flask, diluting the solution with 3-methyl-1-butanol up to the mark on the flask.  Using a spectrophotometer, the chemist finds the percent transmittance of the final 3-methyl-1-butanol solution in a 2.00-cm cuvet is 18.8 at 454 nm.  The chemist then prepares the sample.  She treats 0.2990 g of the previously dried copper oxide sample with a minimum volume of concentrated sulfuric acid in order to get all of the copper into solution (aqueous) as copper(II) ions.  After neutralizing the copper-containing solution with base, the chemist transfers the solution quantitatively to a 500.0-mL volumetric flask and then dilutes the solution with deionized water up to the mark on the flask.  Next, the chemist treats 10.00 mL of the solution with the reducing agent and then adds the buffer.  Subsequently, the chemist treats the resulting solution with neocuproine and then adds 100.00 mL of 3-methyl-1-butanol.  After shaking well to make sure that essentially all of the Cu(ncup)₂⁺ is extracted by the 3-methyl-1-butanol from the aqueous solution, the chemist separates the aqueous layer (bottom) completely from the 3-methyl-1-butanol layer (top) and then quantitatively transfers the 3-methyl-1-butanol layer to a 500.0-mL volumetric flask, diluting the solution with 3-methyl-1-butanol up to the mark on the flask.  Using a spectrophotometer, the chemist finds the percent transmittance of the final 3-methyl-1-butanol solution in a 2.00-cm cuvet is 27.6 at 454 nm.  Find the percent by mass of copper in the sample analyzed by the analytical chemist.