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What is the correct cell notation for the redox reaction 3Pb2 plus aq plus 2Cr s 3Pb s plus 2Cr3 plus aq?
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∙ 14y ago
Cr(s) | Cr3+(aq) Pb2+(aq) | Pb(s)
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∙ 14y ago
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What element is reduced in this reaction cr2o7 3hno2 5h-2cr3 3no3 4h2o?
In this reaction, chromium (Cr) is being reduced from a +6 oxidation state in Cr2O7 to a +3 oxidation state in 2Cr3+.
Reaction between potassium dichromate and iron sulphate?
When potassium dichromate reacts with iron (II) sulfate in an acidic solution, a redox reaction occurs. The dichromate ions are reduced to chromium (III) ions, while iron (II) ions are oxidized to iron (III) ions. The overall reaction is 6Fe2+ + Cr2O72- + 14H+ -> 6Fe3+ + 2Cr3+ + 7H2O.
Write a balanced redox equation for the oxidation of chloride to chlorine by acidified potassium dichromate?
K2Cr2O7 + 4H2SO4 + 6Cl-1----------> K2SO4 + Cr2(SO4)3 + 3Cl2 + 4H2O + 3O-2
What is the Reaction of k2cr2o7 with so2?
The reaction of K2Cr2O7 with SO2 in acidic medium results in the formation of chromium(III) sulfate (Cr2(SO4)3), sulfuric acid (H2SO4), and water. This reaction involves the reduction of Cr(VI) in K2Cr2O7 to Cr(III) in chromium(III) sulfate.
Chemical reaction between iron and potassium dichromate?
When iron reacts with potassium dichromate, iron(II) ion is oxidized to iron(III) ion by dichromate, which gets reduced to chromium(III) ion. The balanced chemical equation for this reaction is: 6 Fe^2+ + 14 H^+ + Cr2O7^2- --> 6 Fe^3+ + 2 Cr^3+ + 7 H2O
Disproportionation of chromium oxide in acid?
In acidic conditions, chromium(III) oxide undergoes disproportionation, forming chromium(II) ions and chromium(VI) ions. The overall reaction is: 2Cr2O3 + 4H+ -> 2Cr3+ + Cr2O7^2- + 2H2O
What is the correct formula for the ionic compound formed between chromium and chloride?
The correct formula for the ionic compound formed between chromium and chloride is CrCl3. This is because chromium has a 3+ charge and chloride has a 1- charge, so it takes three chloride ions to balance the charge of one chromium ion.
What is the reaction between dichromate and iodide?
When dichromate reacts with iodide ions in acidic solution, chromium is reduced from a +6 oxidation state to a +3 oxidation state, and iodide is oxidized to iodine. The balanced equation for this reaction is: Cr2O7 2- + 6I- + 14H+ → 2Cr3+ + 3I2 + 7H2O
What is the reaction of acidified pot dichromate with Hydrogen Sulphide?
When acidified potassium dichromate (K2Cr2O7) reacts with hydrogen sulfide (H2S), it forms chromium(III) sulfide (Cr2S3), sulfur dioxide (SO2), and water (H2O). The orange dichromate solution turns green as Cr2S3 is formed. This reaction is often used as a test for the presence of hydrogen sulfide gas.
What is the new oxidation number for cr2o7-2 plus 8h plus 3so3-2 2cr3 plus 3sov-2 plus 4h20?
The new oxidation number for Cr2O7^2- is +6, for H is +1, for SO3^2- is +4, for Cr3+ is +3, for SO4^2- is +6, and for H2O is 0.
What is the net ionic equation for chromium sulfate and ammonium carbonate Cr2SO43 NH42CO3also what are the spectator ions of this equation?
The net ionic equation for the reaction between chromium sulfate (Cr2(SO4)3) and ammonium carbonate (NH4)2CO3 is: Cr2(SO4)3 + 3(NH4)2CO3 -> 2Cr(CO3)3 + 3(NH4)2SO4 The spectator ions in this reaction are NH4+ and SO4^2-.
How many milliliters of 0.325 N HCl are nescessary to reduce 37.6 milliliters of a 0.526 N solution of K2Cr2O7?
To calculate the volume needed, we can use the equation M1V1 = M2V2 where M1 is the concentration of HCl, V1 is the volume of HCl, M2 is the concentration of K2Cr2O7, and V2 is the volume of K2Cr2O7. Plugging in the values, we get (0.325)(V1) = (0.526)(37.6). Solving for V1, the volume of 0.325 N HCl needed is approximately 64.52 mL.
