Homework Answers
The structure of the carbonated Mn is the MnCO3
Now oxygen hase oxidation no. is -2 and C oxidation no. is +4
So
Oxidation state of the Mn + Oxidation state of the C + 3 * Oxidation state of the O = 0
Oxidation state of the Mn + 4 - 3(2) = 0
Oxidation state of the Mn + 4-6 = 0
Oxidation state of the Mn = 2
So oxydation state of Mn is +2 in the sampel
After thremal decompostion
2 MnCO3 (s) + O2 (g) --------> 2 MnO2 (s) +2CO2 (g)
In the Product, it is
Oxidation state of the Mn +2 * Oxidation state of the O = 0
Oxidation state of the Mn +2*(-2) = 0
Oxidation state of the Mn = 4
So in product after thermal decompositon oxydation of Mn is +4
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2.50 g of a pure sample of a carbonate of manganese produces 0.5367 g of CO2...
a. b. Complete and balance the following molecular equations. Write the net ionic equations. To receive...
a. b. Complete and balance the following molecular equations. Write the net ionic equations. To receive full credit, you must indicate the form of each product as (s). (1, (g) or (aq). (12 pts.) - Al(CIO4)3(aq) + Na2CO3(aq) Ba(OH)2(aq) +_ HI(aq) → _CuCl2 (aq) + _ Zn(s) - Cobalt(II) nitrate is used to make catalysts for the synthesis of hydrocarbons from carbon monoxide and hydrogen. 18.189 g of cobalt(II) nitrate hexahydrate (FW 291.03 g/mole) is dissolved in water to the...
Question 2 (2 points) A 3.2100-g sample of a salt was analyzed for its chloride content...
Question 2 (2 points) A 3.2100-g sample of a salt was analyzed for its chloride content as follows: the entire sample was dissolved with distilled water in a 500.0-ml volumetric flask. A 100.00-mL aliquot of the solution required 24.89-mL of a 0.03769 M silver nitrate solution to reach equivalence. A blank correction was not required. Calculate the % (w/w) chloride in the sample. The net-ionic equation for the reaction is Ag*(aq) + CI (aq) - AgCl(s). Provide your answer to...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
please write properly,asking 2.times 3) 2.413 g sample contains Na CO2, NaHCO, and inert material. This...
please write properly,asking
2.times
3) 2.413 g sample contains Na CO2, NaHCO, and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCI was consumed. Calculate the percentage of NaHCO, and Na...
When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperatur...
When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 degrees C to 16.9 degrees C. Calculate Delta H kJ/mol NH4NO3 for the solution process NH4NO3 ( s) yields NH4 (there is a plus sign above the four)(aq) + ^ + NO3(negative sign above the three) (aq) Assume that the specific heat of the solution is the same as that of pure water. Express your answer...
When a 6.07-g sample of solid lead(II) nitrate dissolves in 31.9 g of water in a...
When a 6.07-g sample of solid lead(II) nitrate dissolves in 31.9
g of water in a coffee-cup calorimeter (see above figure) the
temperature falls from 22.00 oC to 18.47 oC.
Calculate H in kJ/mol Pb(NO3)2 for
the solution process.
Pb(NO3)2(s)
Pb2+(aq) + 2 NO3-(aq)
The specific heat of water is 4.18 J/g-K.
Hsolution = ?kJ/mol
Pb(NO3)2.
A 0.6739 g sample of a pure carbonate, X,CO,(s), was dissolved in 50.0 mL of 0.1850 M HCl(aq). The excess HCl(aq)...
A 0.6739 g sample of a pure carbonate, X,CO,(s), was dissolved in 50.0 mL of 0.1850 M HCl(aq). The excess HCl(aq) was back titrated with 24.70 mL of 0.0980 M NaOH(aq). How many moles of HCl react with the carbonate? moles of HCI = mol What is the identity of the cation, X? cation: A standardized solution that is 0.0100 M in Na+ is necessary for a Hame photometric determination of the element. How many grams of primary-standard-grade sodium carbonate...
A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution....
A 1.04 g sample of KBr is dissolved in water to give 155 mL of
solution. This solution is then added to 165 mL of 0.015 M aqueous
Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the
solution via precipitation as insoluble PbBr2(s).
The precipitation reaction that occurs is: Pb2+ (aq) + 2 Br (aq)
---> PbBr2 (s)
At the end of the reaction, what is the concentration (in
molarity) of nitrate ions in the solution?
Note:...
xamination, Long Question 2 2.1 The purity of a sample of solid potassium cyanide is determined...
xamination, Long Question 2 2.1 The purity of a sample of solid potassium cyanide is determined as follows: • 5.00 g of impure potassium cyanide is weighed off and transformed into to a 100.00 ml. volumetric flack, dissolved and made up to the mark. • A 10.00 ml. portion of this solution is pipetted into a conical flask, and titrated with 0.700 M KMnO solution • The average titrwtion value wa 20,69 ml of the KM The reaction stoichiometry is...
Question 1 (1 point) A 52.30 g sample of Ba(OH)2 is dissolved in enough water to...
Question 1 (1 point) A 52.30 g sample of Ba(OH)2 is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 M Ba(OH)2? 62.8 mL 254 mL O 305 ml O 523 mL O 393 mL O Question 2 (1 point) A chemist needs 225 mL of 2.3 M HCl. What volume of 12 M HCl must be dissolved in water...
a. b. Complete and balance the following molecular equations. Write the net ionic equations. To receive full credit, you must indicate the form of each product as (s). (1, (g) or (aq). (12 pts.) - Al(CIO4)3(aq) + Na2CO3(aq) Ba(OH)2(aq) +_ HI(aq) → _CuCl2 (aq) + _ Zn(s) - Cobalt(II) nitrate is used to make catalysts for the synthesis of hydrocarbons from carbon monoxide and hydrogen. 18.189 g of cobalt(II) nitrate hexahydrate (FW 291.03 g/mole) is dissolved in water to the...
Question 2 (2 points) A 3.2100-g sample of a salt was analyzed for its chloride content as follows: the entire sample was dissolved with distilled water in a 500.0-ml volumetric flask. A 100.00-mL aliquot of the solution required 24.89-mL of a 0.03769 M silver nitrate solution to reach equivalence. A blank correction was not required. Calculate the % (w/w) chloride in the sample. The net-ionic equation for the reaction is Ag*(aq) + CI (aq) - AgCl(s). Provide your answer to...
please write properly,asking
2.times
3) 2.413 g sample contains Na CO2, NaHCO, and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCI was consumed. Calculate the percentage of NaHCO, and Na...
When a 6.07-g sample of solid lead(II) nitrate dissolves in 31.9
g of water in a coffee-cup calorimeter (see above figure) the
temperature falls from 22.00 oC to 18.47 oC.
Calculate H in kJ/mol Pb(NO3)2 for
the solution process.
Pb(NO3)2(s)
Pb2+(aq) + 2 NO3-(aq)
The specific heat of water is 4.18 J/g-K.
Hsolution = ?kJ/mol
Pb(NO3)2.
A 0.6739 g sample of a pure carbonate, X,CO,(s), was dissolved in 50.0 mL of 0.1850 M HCl(aq). The excess HCl(aq) was back titrated with 24.70 mL of 0.0980 M NaOH(aq). How many moles of HCl react with the carbonate? moles of HCI = mol What is the identity of the cation, X? cation: A standardized solution that is 0.0100 M in Na+ is necessary for a Hame photometric determination of the element. How many grams of primary-standard-grade sodium carbonate...
A 1.04 g sample of KBr is dissolved in water to give 155 mL of
solution. This solution is then added to 165 mL of 0.015 M aqueous
Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the
solution via precipitation as insoluble PbBr2(s).
The precipitation reaction that occurs is: Pb2+ (aq) + 2 Br (aq)
---> PbBr2 (s)
At the end of the reaction, what is the concentration (in
molarity) of nitrate ions in the solution?
Note:...
xamination, Long Question 2 2.1 The purity of a sample of solid potassium cyanide is determined as follows: • 5.00 g of impure potassium cyanide is weighed off and transformed into to a 100.00 ml. volumetric flack, dissolved and made up to the mark. • A 10.00 ml. portion of this solution is pipetted into a conical flask, and titrated with 0.700 M KMnO solution • The average titrwtion value wa 20,69 ml of the KM The reaction stoichiometry is...
Question 1 (1 point) A 52.30 g sample of Ba(OH)2 is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 M Ba(OH)2? 62.8 mL 254 mL O 305 ml O 523 mL O 393 mL O Question 2 (1 point) A chemist needs 225 mL of 2.3 M HCl. What volume of 12 M HCl must be dissolved in water...
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