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fuchsiawombat5Lv1

24 Jun 2021

Question 1

Name the substances and arrange the oxidation states for all the elements

Potassium chlorate, Na2SO3, Fe(H2PO4)3, K2Cr2O7, hydrogen peroxide, metaphosphoric acid

Question 2

Describe the chemical properties of the salts.

Find the mass of the precipitate that is formed by the reaction of 50 grams of copper (II) chloride with an excess of potassium hydroxide.

Question 3

Make up the equations of reactions occurring in an aqueous solution. Select the coefficients using half-reactions:

K2Cr2O7 KNO2 H2SO4 =

Al H2SO4 (diluted) =

KMnO4 H2S H2SO4 =

Question 4

Calculate the volume of the released gas during the reaction of 5 grams of copper with concentrated sulfuric acid.

Question 5

Find the mass of the precipitate during the reaction of 5 grams of potassium iodide with 5 grams of potassium nitrate in an acidic medium.

Question 6

46 element of the periodic table.

Write a full and abbreviated electronic form for it. Write an abbreviated formula for an ion with a charge of 2

Write the quantum numbers for the last electron that is filled in this atom.

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14 Apr 2022

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Can I get all of the question answered in a way that I know under which sub question the answer goes please.

Can I get all of the questions answered in a way that I know how it fits in the question. Some parts are explanations. Thank you.

Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bubbles, and the pink solution was turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese (II) sulfate; water was also formed during the same reaction. Please answer the followings:

1) Write down the balanced chemical equation for this reaction.

2) Define the type/types of the reaction; assign the oxidation number of Manganese in potassium permanganate and manganese (II) sulfate. Also, offer an explanation for the color change.

3) Write down the ions present in the solution before & after the reaction. If 100 mL 0.5 M potassium permanganate was mixed with 50 mL 2 M sulfuric acid, what will be the final pH (>7 or <7) of the solution?

4) After the completion of reaction, when evolution of gas-bubbles ceased, what will happen if an aqueous solution of sodium carbonate was added to the reaction mixture? Please write down the net ionic equation.

5) If initially 5.65 g of potassium permanganate was taken for the reaction, calculate the total mass of manganese (II) sulfate present in the solution after the completion of the reaction. What is the Manganese ion concentration of the solution (assume that the total volume of the final reaction mixture is 500 mL)?

Useful hints: hydrogen peroxide is a strong oxidizing agent and considered to be a molecular compound.

(2) Citric acid (H3C6H5O7) occurs in plants. The acid is added to beverages and candy. An aqueous solution is 0.710 m in citric acid. The density is 1.049 g/mL. Calculate the concentration of this solution as: (w/w %) (w/v %) M Mole Fraction (citric acid) 2

(3) When 75.0 mL of a 0.100 M lead (II) nitrate solution is mixed with 100.0 mL of a 0.190 M potassium iodide solution, a yellow-orange precipitate of lead (II) iodide is formed. a. Write the balanced molecular and net-ionic equation. b. Assuming 100% yield calculate the mass of lead (II) iodide formed. c. Determine the molarities of ions left in solution after the reaction.

(4) A 15.00 mL solution of KNO3 was diluted to 125.0 mL and 25.00 mL of this solution was then diluted to 1000. mL. The concentration of KNO3 in the 1000. mL is 0.00383 M. What was the M of KNO3 in the original solution? 3

(5) How many grams of pure H2SO4 can be obtained from 250 g of iron ore if the ore is 82.0 % (w/w %) FeS2. The reactions involved are given below: 4FeS2 + 11O2 â 2Fe2O3 + 8SO2 (95.0% efficient) 2SO2 + O2 â 2SO3 (90.0 % efficient) SO3 + H2O â H2SO4 (90.0 % efficient)

(6) 30.0 mL of 0.512 M sulfuric acid was added to 25.0 mL of 0.666 M sodium hydroxide. a. Write the balanced chemical equation. b. Determine the molarity of either acid or base remaining after the reaction. c. Find the molarity if a 50.00 mL aliquot of this solution is diluted to 250. mL.

(8) Oxygen is produced by the reaction: 2KClO3 (s) â2KCl (s) + 3O2 (g) ï· The oxygen produced was collected over water. A sample of KClO3 produced 705 mL of oxygen saturated with water vapor at 20.0 Â°C where the vapor pressure of water is 17.54 mm Hg. The total gas pressure was 1.104 atm. What mass of KClO3 decomposed?

(9) How many grams of C2H2 must burn according to the equation below in order to heat 2.34 Ã 104 g of H2O from 25.0 Â°C to 35.0 Â°C? C2H2 (g) + O2 (g) âH2O (l) + CO2 (g), Î = â 1212 kJ

Iâve attached the lab procedures

Could I get some help with the questions please

Weigh boat is 2.20g

Weigh boat + copper is 2.43g