When native ore of gold treated with aqueous solution of NaCN in the presence of oxygen then which of the following property is not related with the formed complex.sp3 hybridizedDiamagneticGold is in +1 oxidation stateMaximum number of atom in one plane is 5

smuggler could not carry gold by depositing iron on the gold surface sincegold is densergold has higher reduction potential than irongold has lower reduction potential than ironNone of these

Which of the following ore(s) contain oxygen atom?

Ore is a naturally occuring rock found in Earth's crust that contains valuable minerals and metals.  In an experiment, a researcher dissolved a sample of ore containing an unknown amount of iron in HCl(aq).  The resulting aqueous solution, which contained both Fe2+(aq) and Fe3+(aq), was poured through a Jones reductor column containing Zn(Hg)(s) to convert all iron ions into a single oxidation state.  The conversion of Fe3+(aq) to Fe2+(aq) in the Jones reductor column is shown in Figure 1.Figure 1  Jones reductor column used for the conversion of Fe3+(aq) to Fe2+(aq).  The resulting Fe2+(aq) solution was collected using a syringe.To determine the total amount of iron in the sample, the Fe2+(aq) solution was then transferred to a container and titrated with 0.1 M K2Cr2O7(aq), which resulted in the conversion of Fe2+(aq) to Fe3+(aq) in an irreversible process.  A reference electrode was used to monitor the solution potential as a function of K2Cr2O7(aq) volume added, and the equivalence point of the solution was reached after the addition of 9.50 mL of K2Cr2O7(aq).  A schematic of the experimental setup is shown in Figure 2.Figure 2  Experimental setup for the titration of Fe2+(aq) with K2Cr2O7(aq) under acidic conditionsIn a second experiment, the researcher prepared another sample of Fe2+(aq) but used a 0.1 M I3−(aq) titrant solution instead of K2Cr2O7(aq).The standard reduction potentials for the species involved in the experiments are given in Table 1.Table 1  Standard reduction potentialsReduction half-reaction E°(V)Cr2O72−(aq) + 14 H+(aq) + 6 e− → 2 Cr3+(aq) + 7 H2O(l) +1.33Fe3+(aq) + e− → Fe2+(aq) +0.76I3−(aq) + 2 e− → 3 I−(aq) +0.53Zn2+(aq) + Hg(l) + 2 e− → Zn(Hg)(s) −0.76 Question 26Does the redox reaction between Cr2O72−(aq) and Fe2+(aq) require energy input?A.Yes; ∆G° = +2.09nF J/mol.B.Yes; ∆G° = +0.57nF J/mol.C.No; ∆G° = −0.57nF J/mol.D.No; ∆G° = −2.09nF J/mol.

Ore is a naturally occuring rock found in Earth's crust that contains valuable minerals and metals.  In an experiment, a researcher dissolved a sample of ore containing an unknown amount of iron in HCl(aq).  The resulting aqueous solution, which contained both Fe2+(aq) and Fe3+(aq), was poured through a Jones reductor column containing Zn(Hg)(s) to convert all iron ions into a single oxidation state.  The conversion of Fe3+(aq) to Fe2+(aq) in the Jones reductor column is shown in Figure 1.Figure 1  Jones reductor column used for the conversion of Fe3+(aq) to Fe2+(aq).  The resulting Fe2+(aq) solution was collected using a syringe.To determine the total amount of iron in the sample, the Fe2+(aq) solution was then transferred to a container and titrated with 0.1 M K2Cr2O7(aq), which resulted in the conversion of Fe2+(aq) to Fe3+(aq) in an irreversible process.  A reference electrode was used to monitor the solution potential as a function of K2Cr2O7(aq) volume added, and the equivalence point of the solution was reached after the addition of 9.50 mL of K2Cr2O7(aq).  A schematic of the experimental setup is shown in Figure 2.Figure 2  Experimental setup for the titration of Fe2+(aq) with K2Cr2O7(aq) under acidic conditionsIn a second experiment, the researcher prepared another sample of Fe2+(aq) but used a 0.1 M I3−(aq) titrant solution instead of K2Cr2O7(aq).The standard reduction potentials for the species involved in the experiments are given in Table 1.Table 1  Standard reduction potentialsReduction half-reaction E°(V)Cr2O72−(aq) + 14 H+(aq) + 6 e− → 2 Cr3+(aq) + 7 H2O(l) +1.33Fe3+(aq) + e− → Fe2+(aq) +0.76I3−(aq) + 2 e− → 3 I−(aq) +0.53Zn2+(aq) + Hg(l) + 2 e− → Zn(Hg)(s) −0.76 Question 28What happens to the chromium atoms in K2Cr2O7(aq) during the titration in the passage?A.Cr6+ is oxidized to Cr3+B.Cr7+ is oxidized to Cr3+C.Cr6+ is reduced to Cr3+D.Cr7+ is reduced to Cr3+

Ore is a naturally occuring rock found in Earth's crust that contains valuable minerals and metals.  In an experiment, a researcher dissolved a sample of ore containing an unknown amount of iron in HCl(aq).  The resulting aqueous solution, which contained both Fe2+(aq) and Fe3+(aq), was poured through a Jones reductor column containing Zn(Hg)(s) to convert all iron ions into a single oxidation state.  The conversion of Fe3+(aq) to Fe2+(aq) in the Jones reductor column is shown in Figure 1.Figure 1  Jones reductor column used for the conversion of Fe3+(aq) to Fe2+(aq).  The resulting Fe2+(aq) solution was collected using a syringe.To determine the total amount of iron in the sample, the Fe2+(aq) solution was then transferred to a container and titrated with 0.1 M K2Cr2O7(aq), which resulted in the conversion of Fe2+(aq) to Fe3+(aq) in an irreversible process.  A reference electrode was used to monitor the solution potential as a function of K2Cr2O7(aq) volume added, and the equivalence point of the solution was reached after the addition of 9.50 mL of K2Cr2O7(aq).  A schematic of the experimental setup is shown in Figure 2.Figure 2  Experimental setup for the titration of Fe2+(aq) with K2Cr2O7(aq) under acidic conditionsIn a second experiment, the researcher prepared another sample of Fe2+(aq) but used a 0.1 M I3−(aq) titrant solution instead of K2Cr2O7(aq).The standard reduction potentials for the species involved in the experiments are given in Table 1.Table 1  Standard reduction potentialsReduction half-reaction E°(V)Cr2O72−(aq) + 14 H+(aq) + 6 e− → 2 Cr3+(aq) + 7 H2O(l) +1.33Fe3+(aq) + e− → Fe2+(aq) +0.76I3−(aq) + 2 e− → 3 I−(aq) +0.53Zn2+(aq) + Hg(l) + 2 e− → Zn(Hg)(s) −0.76 Question 27The net reaction occurring in the Jones reductor column is:A.Fe3+(aq) + Zn(Hg)(s) + e− → Fe2+(aq) + Zn2+(aq) + Hg(l) + 2 e−B.Fe3+(aq) + Zn2+(aq) + Hg(l) → Fe2+(aq) + Zn(Hg)(s)C.2 Fe3+(aq) + Zn(Hg)(s) → 2 Fe2+(aq) + Zn2+(aq) + Hg(l)D.2 Fe3+(aq) + Zn(Hg)(s) + 2 e− → 2 Fe2+(aq) + Zn2+(aq) + Hg(l) + 2 e−