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When elemental iron corrodes it combines with oxygen in the air to ultimately form red brown iron(III) oxide which we call rust. (a) If a shiny iron nail with an initial mass of 23.2 g is weighed after being coated in a layer of rust, would you expect the mass to have increased, decreased, or remained the same? Explain. (b) If the mass of the iron nail increases to 24.1 g, what mass of oxygen combined with the iron?
a) increase b) 0.9 $\mathrm{g}$
Chemistry 101
Chapter 1
Essential Ideas
Intro to Chemistry
University of Central Florida
Rice University
University of Maryland - University College
Lectures
02:29
Chemistry is the science o…
04:42
In chemistry and physics, …
01:37
Iron metal reacts with oxy…
03:31
If steel wool (iron) is he…
03:53
03:52
Iron reacts slowly with ox…
09:40
The balanced equation for …
03:21
02:23
Iron(III) oxide reacts wit…
05:57
When the supply of oxygen …
02:42
03:03
An iron bar weighed 664 g.…
01:05
Two of the more common oxi…
06:40
Iron reacts with oxygen as…
02:34
01:15
Rusting occurs due to the …
Iron reacts rapidly with c…
00:14
A $56-g$ sample of iron re…
02:38
16:44
In the thermite reaction, …
03:19
Iron ore is converted to i…
02:31
Iron ores, usually oxides …
love one. This is Ricky and today, working on Problem 23. So we have a situation where we have elemental iron that is going to be combining with oxygen and to corrode into iron three oxide. And this is our chemical equation. And so if we start with a mass of iron that's equal to 23.2 grams and then some time passes and we have rust, we will see an increase in the mess posted nail. That's because of three reaction it's had with oxygen. And what would be the mass of the oxygen that combined with the iron Well, we could just do 24.1 rams, which is the new Mass minus 23.2 grams, which is the original Mass and get they 0.9 grams of oxygen combined. So hope this video is helpful. Seeing the
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