Redox-Flow Batteries: From Metals to Organic Redox- Active ...
Redox exercise
2
Classify each of these reactions as a synthesis, decomposition, combustion or a single-displacement reaction. Balance it if you are able. a. NaH Na + H 2 b. KI + Cl 2 KCl + I 2 c. C 2 H 5 SH + O 2 CO 2 + H 2 O + SO 2 d. H 2 + CuO Cu + H 2 O e. P 4 + O 2 P 4 O 10 f. B + O 2 B 2 O 3 g. (C 2 H 5 O) 2 O + O 2 CO 2 + H 2 O h. Cr 2 O 3 + Si Cr + SiO 2 i. NaHCO 3 Na 2 CO 3 + H 2 O + CO 2 Water and carbon dioxide fire extinguishers should not be used on magnesium fires because both substances react with magnesium and generate enough heat to intensify the fire. Determine the oxidation number for each atom in the equations that describe these reactions (displayed below), and decide whether each reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent. Determine the oxidation number for the atoms of each element in the following formula a. HPO 4 2- b. NiSO 4 c. N 2 O 4 2— d. Mn 3 (PO 4 ) 2 e. ClF 3 f. H 2 O 2 g. H 2 SO 4 h. NH 3 Determine whether these reactions are redox reactions, if that is the case, write the oxidation and reduction half reactions and indicate the oxidizing and reducing agents. a. CaO + SO 2 CaSO 3 b. Fe + CuSO 4 FeSO 4 + Cu c. Zn + HCl ZnCl 2 + H 2 d. KI + Pb(NO 3 ) 2 KNO 3 + PbI 2 e. HNO 3 + NaOH H 2 O + NaNO 3 f. Fe + S 8 FeS
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Redox exercise
Transcript of Redox exercise
Classify each of these reactions as a synthesis, decomposition, combustion or a single-displacement reaction. Balance it if you are able.a. NaH Na + H2b. KI + Cl2 KCl + I2c. C2H5SH + O2 CO2 + H2O + SO2d. H2 + CuO Cu + H2Oe. P4 + O2 P4O10f. B + O2 B2O3g. (C2H5O)2O + O2 CO2 + H2Oh. Cr2O3 + Si Cr + SiO2i. NaHCO3 Na2CO3 + H2O + CO2
Water and carbon dioxide fire extinguishers should not be used on magnesium fires because both substances react with magnesium and generate enough heat to intensify the fire. Determine the oxidation number for each atom in the equations that describe these reactions (displayed below), and decide whether each reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.
Determine the oxidation number for the atoms of each element in the following formulaa. HPO42-b. NiSO4c. N2O42d. Mn3(PO4)2e. ClF3f. H2O2g. H2SO4h. NH3
Determine whether these reactions are redox reactions, if that is the case, write the oxidation and reduction half reactions and indicate the oxidizing and reducing agents.a. CaO + SO2 CaSO3b. Fe + CuSO4 FeSO4 + Cuc. Zn + HCl ZnCl2 + H2d. KI + Pb(NO3)2 KNO3 + PbI2e. HNO3 + NaOH H2O + NaNO3 f. Fe + S8 FeSg. ZnO + C Zn + CO2h. Co + Cl2 CoCl2
