1. Redox reactions are characterized by the fact that electrons are between reac
ID: 1038465 • Letter: 1
Question
1. Redox reactions are characterized by the fact that electrons are between reactants A substance which is oxidized electrons and the oxidation number A substance which is reduced electrons and the oxidation number 2. A substance which is an oxidizing agent (Circle one) a. would take electrons from another substance and so be reduced b. would take electrons from another substance and so be oxidized c. would give electrons to another substance and so be reduced d. would give electrons to another substance and so be oxidized 3. To test the relative strength of tin and zinc as oxidizing agents, the following reactions are performed like something is growing on its surface remains shiny Tin(II) sulfate zinc metal we observe that the zinc becomes dark and looks Zinc(lI) sulfate + tin metal- no changes to the tin are observed; its surface (a) Why can only one of the reactions actually occur? (b) Which species is the better oxidizing agent? (Circle one) Sn2+ Zn2+ SO42 Zn 4. Iron reacts with H2SO4 to form iron(Il) sulfate and hydrogen. What species is reduced? (Circle one) a) H2SO4 b) Fe c)H d) Fe2 e) S042 5. How is the free halogen (i.e. Cl2, Br2, or l2) detected in Part B? 6. Why will Br ion never be an oxidizing agent?Explanation / Answer
1) exchanged , looses, increases, gain, decreases.
2) A substance that acts as oxidizing agent causes oxidation in other species and itself gets reduced. So, option 'a' is correct.
3) tendency of an element to displace from it's salt solution depends on it's electrode potential value. The one having highly negative value of reduction potential acts as a strong oxidizing agent whereas high positive value of reduction potential acts as reducing agent. Also , displacement depends on the position of a particular element in the reactivity series. From the equation we can depict that ' zinc is more reactive than tin and is able to displace Tim from it's salt solution. In equation 1 we can see that zinc (0) oxidisesto zinc(2) sulphate and reduces Sn (2) to Sn( 0) . Therefore Zn acts as reducing agent .
In equation 2 ,tin is unable to cause any reaction in zinc .hence it is present below zinc in reactivity series.
b) Sn(2) is an oxidizing agent in the reaction. Because it causes oxidation in Zn .
4) H+ ( H2SO4) is reduced to H2 ( hydrogen gas).
6) Br- has 8 electrons in it's outermost shell( which is it's maximum of any element) ,so it will never acts as an oxidizing agent because it cannot accept electrons further.
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