(v) Complete the process of iron rusting by filling the blanks. Suggest a way to prohibit the process.
The iron rust is formed due to
reaction. Different regions on
iron surface become anode and cathode.
• Reaction on anode region :
Fee
- Fe2+
(aq)
+ 2e -
• Reaction on cathode region :
O2(g) + 4H+ +
(aq)
→ 2H,0a)
When Fe 2+ ions migrate from anode region they react with
form Fe3+ ions.
... to
A reddish coloured hydrated oxide is formed from ..
ions. It is called
rust.
2Fe3+
(aq)
+ 4H,00
→ +
+
(aq)
A way to prevent rusting
-
-
1
#​

219 grams of iron (iii) oxide reacts with excess carbon according to the reaction equation shown below. fe2o3 + c → fe + co2 after a scientist performs the chemical reaction they find the actual yield of iron to be 57.4 grams. calculate the percent yield of this chemical reaction.

Calcium chloride +gold(1) oxide—>

Modern pennies are composed of zinc coated with copper. a student determines the mass of a penny to be 2.482 g and then makes several scratches in the copper coaling (to expose the underlying zinc). the student puts the scratched penny in hydrochloric acid, where the following reaction occurs between the zinc and the hcl (the copper remains undissolved): zn(s) + 2 hcl(aq) → h2(g) + zncl(aq)the student collects the hydrogen produced over water at 25 °c. the collected gas occupies a volume of 0.899 l at a total pressure of 79 j mmhg. calculate the percent zinc (by mass) in the penny. (assume that all the zn in the penny dissolves.)