Make the equations of redox reactions.

In these reactions, hydrogen often exhibits the properties of a reducing agent, that is, it donates electrons. Metals exhibit the properties of reducing agents, donate valence electrons. Let’s compose electronic equations:
A) H2 + CL2 = 2HCL;
2H – 2e = 2H + | 1 – reducing agent;
2CL + 2e = 2CL- | 1 – oxidizing agent.
B) H2 + CrO = Cr + H2O;
2H – 2e = 2H + | 1- reducing agent;
Cr2 + + 2e = Cr | 1- oxidizing agent.
B) H2 + S = H2S;
2H – 2e = 2H + | 1- reducing agent;
S + 2e = S2- | 1- oxidizing agent.
D) 2 Na + H2 = 2NaH;
2Na – 2e = 2Na + | 1 – reducing agent;
2H + + 2e = 2H- | 1- oxidizing agent.
Hydrogen as an oxidizing agent.