Use the following data to work through problems 4-6.

• 50.0 mL of each solution was used in each experiment.
• Each solution had a molarity of 2.00 M.
• The density of the solutions once mixed are 1.03 g/mL.
• The following table is data collected from an actual experiment.

1. Calculate the amount of heat energy, q_surroundings, produced in each reaction. Use 03 g/mL for the density of all solutions. Use the specific heat of water, 4.184 J/(g•°C), for each of the three reactions. q_surroundings = C_s ´ m ´ ∆T

2. Calculate the enthalpy change, ∆H_reaction, per mole of reactant for each of the three reactions in units of kJ/mole.

                                    ∆H_reaction = ∆H_system

3. Calculate a percent error between the accepted values for ∆H_reaction(use values calculated in question 1 as accepted values) and the “experimental” values you calculated in question 5 for each reaction.

                        % Error = Experimental – Accepted x 100

                                                Accepted

A 1.268 g sample of a metal carbonate, MCO33, was treated 100.00 mL of 0.1083 M H22SO44, yielding CO22 gas and an aqueous solution of the metal sulfate. The solution was boiled to remove all of the dissolved CO22 and then was titrated with 0.1241 M NaOH. A 71.02 mL volume of the NaOH solution was required to neutralize the excess H22SO44.

Start by writing a balanced chemical equation for this reaction.

What's the identity of the metal?

Give the elemental symbol

How many grams of CO2 gas were produced?

1) The correct arrangement of the following complex ions in terms of increasing crystal field splitting energy (D) is:

[CrI₆]^3-            [CrF₄]^-            [Cr(en)₃]³⁺            [W(en)₃]³⁺

a) Smallest [CrI₆]^3- < [Cr(en)₃]³⁺ < [CrF₄]^- < [W(en)₃]³⁺ Largest

b) Smallest [CrI₆]^3- < [W(en)₃]³⁺ < [CrF₄]^- < [Cr(en)₃]³⁺ Largest   

c) Smallest [CrF₄]^- < [CrI₆]^3- < [Cr(en)₃]³⁺ < [W(en)₃]³⁺ Largest

d) Smallest [CrF₄]^- < [W(en)₃]³⁺ < [CrI₆]^3- < [Cr(en)₃]³⁺ Largest

e) Smallest [W(en)₃]³⁺ < [Cr(en)₃]³⁺ < [CrF₄]^- < [CrI₆]^3- Largest

2) Determine the number of unpaired electrons for each of the following coordination complexes:

Arrange these complexes in order of increasing number of unpaired electrons (in the answers below an = sign is used if two complexes have the same number of electrons).

a) Fewest [Pt(CN)₄]^2– < [Ni(H₂O)₆]²⁺ < Cr(CO)₆ < [CoCl₆]^2– Greatest

b) Fewest [Pt(CN)₄]^2– = Cr(CO)₆ < [CoCl₆]^2– < [Ni(H₂O)₆]²⁺ Greatest

c) Fewest [Pt(CN)₄]^2– < Cr(CO)₆ < [CoCl₆]^2– < [Ni(H₂O)₆]²⁺   Greatest

d) Fewest [Pt(CN)₄]^2– < Cr(CO)₆ < [Ni(H₂O)₆]²⁺ < [CoCl₆]^2– Greatest

e) Fewest [Pt(CN)₄]^2– = Cr(CO)₆ < [Ni(H₂O)₆]²⁺ < [CoCl₆]^2– Greatest

The pH of solution containing 1 mol Cu(OH)2 in 1L water is 7.66.

Has all the Cu(OH)2 dissolve in water? Ksp=4.8 × 10^-20.

A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.04503 M EDTA solution. The solution is then back titrated with 0.02327 M Zn2 solution at a pH of 5. A volume of 22.80 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the column is treated with 25.00 mL 0.04503 M EDTA. This solution required 21.76 mL of 0.02327 M Zn2 for back titration. The Ni2 extracted from the column was treated witn 25.00 mL of 0.04503 M EDTA. How many milliliters of 0.02327 M Zn2 is required for the back titration of the Ni2 solution?

Benzene as a saturated liquid at 5,000 mmHg is fed to a vaporizer. The product from the vaporizer is a superheat vapor at 165°C and 4,550 mmHg.

For a flow rate of 2,500 moles/min of benzene, how much is needed (kW)?

If steam is available at 500°C and 20 bar and condenses to a saturated liquid at 20 bars, how much steam (kg/hr) is needed to vaporize the benzene?

Know: ΔHv = 30.765 kJ/mol, Tb = 80.10°C, SG = 0.879, Cp (l) = 126.5 * 10^-3 + 23.4 * 10^-5 T (°C), Cp (v) = 74.06 * 10^-3 + 32.95 * 10^-5T - 25.20 * 10^-8 T^2 + 77.57*10^-12 T^3

For the following reaction, 9.88 grams of sulfur are allowed to react with 21.8 grams of carbon monoxide. sulfur (s) + carbon monoxide (g) sulfur dioxide (g) + carbon (s)

What is the maximum amount of sulfur dioxide that can be formed? (in grams)

What is the FORMULA for the limiting reagent?

What amount of the excess reagent remains after the reaction is complete? (in grams)

When 15.0 mL of a 4.89×10^-4 M zinc nitrate solution is combined with 12.0 mL of a 6.25 ×10^-4 M sodium hydroxide solution does a precipitate form?  (yes or no)

For these conditions the Reaction Quotient, Q, is equal to

When 15.0 mL of a 7.41×10^-4M potassium carbonate solution is combined with 12.0 mL of a 4.85×10^-4M copper(II) nitrate solution does a precipitate form?  (yes or no)

For these conditions the Reaction Quotient, Q, is equal to

What do enzymes do and how do they do it (this question is intentionally vague and open ended)?

what effect does ligand exchange cause for cancer therapy?

preferably ruthenium complexes vs platinum complexes

l

2. Determine the mole fraction of zinc(II) sulfite in a 4.22 M aqueous solution of zinc(II) sulfite. The density of the solution is 1.01 g mL^-1. 
answer is not 0.0699

Formic acid (HCOOH) has Ka= 1.8x10-4. What is the pH of a 0.01 M solution of formic acid ?

PLEASE HELP I HAVE EXAM

Complete the following table

1

a) Calculations for orange juice

pH= 4.5

b) calculation for milk

pH= 6.0

Explain why quantum numbers stop following the expected trend for elements at potassium, while they do follow the expected trend for ions.

Find the length and width of a square basin for virus disinfection of a flow of 5 MGD. You may assume a depth of 5 ft, a Cxt product of 20 (mg/L) min for 3-log removal, and a target free chlorine residual of 0.4 mg/L.