a) A0.230 g of liquid compound X containing C, H and O undergoes complete combustion reaction produces 0.270 g of H20. In an analysis, the mass of C in the compound X is found to be 0.120 g. ) Calculate the percentage composition by mass of carbon in compound X. (1] (i) Determine the empirical formuta of compound X. (4) (ii) Write a balanced chemical equation for the reaction above if the molecular formula is the same as empirical formula. (1) (iv) Calculate the percentage yield of CO; if the theoretical mass of COz is 0.520 g. (2} fot In beaker A, aqueous FeCl, is added with excess aqueous silver nitrate, AgNO, yields 7.015 g of a precipitate. Calculate the molarity of chloride ions, Ct in aqueous FeCl, for beaker A if the total volume is 0.250 L (4] et In beaker B, different amount of aqueous FeCl, is titrated with 14.28 ml of 0.1980 M KMNO, and the balanced net ionic equation for the redox reaction is as follows: Mno.taq) + 5 Fe"(aq) + 8 H*(aq) → Mn²"(aq) + 5 Fe*"(aq) + 4 H;0(I) (i) State the oxidation number of manganese in Mno. (1) (i) Identify the number of electrons involved in the redox reaction. [1] (ii) Calculate the number of chloride ions, CI present in beaker B. [3]
a) A0.230 g of liquid compound X containing C, H and O undergoes complete combustion reaction produces 0.270 g of H20. In an analysis, the mass of C in the compound X is found to be 0.120 g. ) Calculate the percentage composition by mass of carbon in compound X. (1] (i) Determine the empirical formuta of compound X. (4) (ii) Write a balanced chemical equation for the reaction above if the molecular formula is the same as empirical formula. (1) (iv) Calculate the percentage yield of CO; if the theoretical mass of COz is 0.520 g. (2} fot In beaker A, aqueous FeCl, is added with excess aqueous silver nitrate, AgNO, yields 7.015 g of a precipitate. Calculate the molarity of chloride ions, Ct in aqueous FeCl, for beaker A if the total volume is 0.250 L (4] et In beaker B, different amount of aqueous FeCl, is titrated with 14.28 ml of 0.1980 M KMNO, and the balanced net ionic equation for the redox reaction is as follows: Mno.taq) + 5 Fe"(aq) + 8 H*(aq) → Mn²"(aq) + 5 Fe*"(aq) + 4 H;0(I) (i) State the oxidation number of manganese in Mno. (1) (i) Identify the number of electrons involved in the redox reaction. [1] (ii) Calculate the number of chloride ions, CI present in beaker B. [3]
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i need help for question (c) (ii) and (iii) , they are not graded questions they are for my revision :(( i'll be having my final exam for chemistry this wednesday please help
![(a) A0.230 g of liquid compound X containing C, H and O undergoes complete combustion reaction produces
0.270 g of H20. In an analysis, the mass of C in the compound X is found to be 0.120 g.
() Calculate the percentage composition by mass of carbon in compound X.
(1]
(ii) Determine the empirical formuta of compound X.
[4]
(ii) Write a balanced chemical equation for the reaction above if the molecular formula is the same as
empirical formula.
(1)
(iv) Calculate the percentage yield of CO2 if the theoretical mass of COz is 0.520 g.
(2]
fot in beaker A, aqueous FeCl, is added with excess aqueous silver nitrate, AgNO, yields 7.015 g of a
precipitate.
Calculate the molarity of chloride ions, Ct in aqueous FeCl, for beaker A if the total volume is 0.250 L
(4)
tet In beaker B, different amount of aqueous FeCl, is titrated with 14.28 mL of 0.1980 M KMNO, and the
balanced net ionic equation for the redox reaction is as follows:
Mno.taq) + 5 Fe"(aq) + 8 H*(aq) → Mn²"(aq) + 5 Fe"(aq) + 4 H;0(1)
(i) State the oxidation number of manganese in Mno.
(1)
(i) Identify the number of electrons involved in the redox reaction.
[1]
(iii) Calculate the number of chloride ions, Cl' present in beaker B.
[3]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F453b2fb0-289a-45e5-a97f-cc442700ead2%2Fbe63a89c-21cf-4f66-a873-8d007258f3b9%2Fpz4wyca_processed.png&w=3840&q=75)
Transcribed Image Text:(a) A0.230 g of liquid compound X containing C, H and O undergoes complete combustion reaction produces
0.270 g of H20. In an analysis, the mass of C in the compound X is found to be 0.120 g.
() Calculate the percentage composition by mass of carbon in compound X.
(1]
(ii) Determine the empirical formuta of compound X.
[4]
(ii) Write a balanced chemical equation for the reaction above if the molecular formula is the same as
empirical formula.
(1)
(iv) Calculate the percentage yield of CO2 if the theoretical mass of COz is 0.520 g.
(2]
fot in beaker A, aqueous FeCl, is added with excess aqueous silver nitrate, AgNO, yields 7.015 g of a
precipitate.
Calculate the molarity of chloride ions, Ct in aqueous FeCl, for beaker A if the total volume is 0.250 L
(4)
tet In beaker B, different amount of aqueous FeCl, is titrated with 14.28 mL of 0.1980 M KMNO, and the
balanced net ionic equation for the redox reaction is as follows:
Mno.taq) + 5 Fe"(aq) + 8 H*(aq) → Mn²"(aq) + 5 Fe"(aq) + 4 H;0(1)
(i) State the oxidation number of manganese in Mno.
(1)
(i) Identify the number of electrons involved in the redox reaction.
[1]
(iii) Calculate the number of chloride ions, Cl' present in beaker B.
[3]
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