State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced.
`Cl_2 + H_2S to 2HCI + S`

State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced. H_2 S + Cl_2 to 2 HCl + S

State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced. PbO + CO to Pb + CO_2

State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced. Mg + 2HCl to MgCl_2 + H_2

State whether the compounds shown in bold letters are oxidised or reduced. Provide reasons also. CuO+H_2 to Cu+H_2O

Indicate in the following reactions which of the reactants, if any, are oxidised or reduced: a. 2HI(aq)+Cl_(2)(aq) rarr I_(2)(s) + 2HCl(aq) b. 2MnO_(2) + 4Al rarr 3Mn +2Al_(2)O_(3) c. 2MnO_(4)^(Ө) + 10Cl^(Ө) + 16H^(o+) rarr 2Mn^(2+) + 5Cl_(2) + 8H_(2)O d. 2Cu^(2+)+2Br^(Ө)+SO_(2)+H_(2)Orarr 2CuBr+4H^(o+)

State giving reason whether the following reaction would involve an increase, a decrease or no change in entropy. 4Fe(s) + 3O_2(g) to 2Fe_2O_3 (s)

With reference to the equation Cl_(2)+H_(2)Sto2HCl+S pertaining to a redox reaction - select the correct answer in each case a. Chlorine is oxidised/reduced to HCl. B. Hydrogen sulphide is oxidised /reduced to sulphur since the reaction involves addition/ removal of hydrogen. c. Chlorine acts as an oxidising / reducing agent.

Name the substance oxidised and the substance reduced, and also identify the oxidising agent and reducing agents in the following reactions : (a) 3MnO_(2) +4Al to 3Mn +2Al_(2)O_(3) (b) Fe_(2)O_(3) + 3CO to 2Fe + 3CO_(2) (c) SO_(2) + 2H_(2)S to 3S +2H_(2)O

Assertion :- In the reaction Zn(s)+cu^(+2)(aq)rarrZn^(+2)(aq)+Cu(s) Cu^(+2) ions act as oxidising agent and Zn atoms act as a reducing agent. Reason :- A substance when readily gain electrons from other, substance is an oxidising agent while reducing agent is a substance which can lose electrons to other susbtances.

Chlorine oxidises H_2 S to