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Which substance is the oxidizing agent in this reaction? - Home Work Help

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Which substance is the oxidizing agent in this reaction? – Home Work Help

Which substance is the oxidizing agent in this reaction? feo+co→fe+co2 express your answer as a chemical formula?

How can you identify the substance being oxidized in the... | Socratic

How can you identify the substance being oxidized in the… | Socratic – In order for a redox reaction to take place, you need equal numbers of electrons lost in the oxidation half-reaction and gained in the reduction half-reaction. You can thus say that methane is acting as a reducing agent because it reduces oxygen gas. Similarly, oxygen gas acts an oxidizing agent…An oxidizing agent causes other chemicals to be oxidized – it is an agent of oxidation! It rips electrons off of other chemicals and takes them for itself…Common Oxidizing Agents and Reducing Agents. In looking at oxidation-reduction reactions, we can focus on the role played by a particular reactant in a chemical reaction. Oxalic acid is oxidized to carbon dioxide in this reaction and the permanganate ion is reduced to Oxidation: H2C2O4. CO2.

9.1 Identify the Oxidizing and Reducing Agents in Redox Equations… – Substance oxidized Fe2+ Reducing agent Fe2+. Oxidizing agent Cr6+ Substance reduced Cr6+. Redox Half Reactions and Reactions WS #2. 5. Circle each oxidizing agent: F- F O2- O2. 6. Ni+2 reacts with Mn, however, Al+3 does not react with Mn. Rank the oxidizing agents in order of…- chemical reaction with water. CO2+H2O→H2CO3 is a substance – carbonic acid is one of the weak acids, it is added to carbonated The most frequent used the word "amphoteric" for the oxides of metals. Example amphoteric oxides can be: ZnO – zinc oxide (white powder, often used in medicine…Carbon monoxide(3CO) is the reducing agent. Reducing agent is an element or a compound that loses electrons. In other words, it is said to be oxidized. In this reaction, 3CO gains oxygen (while reacting with Fe2O3) and becomes 3CO2.

9.1 Identify the Oxidizing and Reducing Agents in Redox Equations...

Oxidizing and Reducing Agents | Oxidation – Reduction Reactions – Oxidizing and reducing agents. This is the currently selected item. half-reaction write the chlorine molecule all right gained those two electrons in magenta so those two electrons in magenta we're going to put over here this time the chlorine molecule and gained them and that turned the chlorine atoms…Fe2O3 + 3 CO → 2 Fe + 3 CO2. Oxidation Iron in Fe2O3 has been reduced in this reaction and has played a role of oxidizing agent by oxidizing carbon from + 2 state to + 4 state.The oxidizing agent is H2SO4 since it causes Cu to be oxidized. What type of reaction is CH4 plus O2 equals CO2 plus H2O? It is a combustion reaction, which is a reaction in which a substance combines with oxygen, releasing a large amount of energy in the form of light and heat.

Solved: Please Write The Answer As A Chemical Formula And ...

AQA AS Redox Lesson 3 – .

Blast Furnace – .

How to predict products for combustion reactions, including hydrocarbon combustion – Hello and welcome to a series of videos
on product prediction in which we will take a look at what products will form
from a given set of reactants.
And in this video among the five reaction types
presented in introductory texts, we will look at product prediction for
combustion. There are two categories we will look at, the first is combustion in
general, and the second is hydrocarbon combustion. Let's begin with combustion
and then consider hydrocarbon combustion. The model for combustion is rapid
reaction with oxygen, and so the identifying feature of a combustion
reaction is that oxygen is a reactant. In particular note that combustion is a
rapid reaction. There are many reactions constantly occurring all around us and
in our bodies that are substances reacting with oxygen, in the air or in
our cells, but these are not combustion. We would notice combustion
immediately because it gives off lots of heat and has a flame, in other words fire.
Fire is another word for combustion. Examples are the combustion of aluminium,
and of carbon. So oxygen is a required reactant, and what is reacting is called
fuel, a common word we use with any fire. There are two subcategories shown here:
The first is combustion of metals, the second is combustion of nonmetals.
Let's first take a look at metals. Most metals will oxidize slowly in air which
is often called corrosion, or rust in the case of oxidized iron. But metals can
burn at high enough temperatures, and/or with a large surface area. For example
powdered aluminum combusts quite readily. The product Al2O3 can be predicted quite
readily from the charges occurring on aluminum and oxygen ions, since the
product of oxygen and any metal is an ionic compound. Aluminum has a 3+
charge while oxygen is 2 -. We need to write subscripts that will balance the
charges, and two aluminum ions will balance the charge of three oxygen ions,
and so the subscripts are 2 and 3. Once the correct product formula is
determined, the equation can then be balanced. Many metals however can have
more than one possible charge, such as most transition metals. For iron the most
stable charge is three plus and so the subscripts required to balance
the combustion of iron and oxygen are 2 and 3, Fe2O3. And then the
equation can be balanced. Under different reaction conditions metals can form less
favorable charges such as 2+ for iron. In this case the product would be FeO with these coefficients. Without knowing
which charge a transition metal will have, assume it will take on the most
stable charge, which can be looked up in a text book or on the internet. Next are
nonmetals. However it is very difficult to predict the products of reactions
between nonmetals. Carbon and oxygen reacting can produce both carbon dioxide
and carbon monoxide. Two of the products of burning sulfur are sulfur dioxide and
sulfur trioxide. Reactions between nonmetals often produce more than one
product, and predicting them requires an understanding of formal charge, Lewis
structures, and optimizing reaction conditions, all of its are beyond the
scope of this video. And so we will turn to our last category the combustion of
hydrocarbons. Like any combustion hydrocarbon combustion requires oxygen.
But here if the other reactant is a hydrocarbon, then the products will be
carbon dioxide and water. So what is a hydrocarbon? Hydrocarbons come in two
slightly different forms. The first one we see here as CxHy the other is CxHyOz,
with the x y and z representing a huge range of subscripts. For example CH4 is
methane or we could have ethane, propane, octane, and waxes have in the vicinity of
24 carbons, and there are many, many more. If any of them react with oxygen, then
the products are carbon dioxide and water. That second type of hydrocarbon
you need to be able to identify is just CxHy that has been oxidized to some
degree, in other words has oxygen in the formula, so that its general formula is
CxHyOz, such as formaldehyde, CH2O, or ethyl alcohol, glycerin, complex
carbohydrates, and thousands of others. They are all hydrocarbons that will
react with oxygen to produce carbon dioxide and water. So you
need to be able to identify a hydrocarbon as having in general the
formula CxHy or CxHyOz. And once you've identified a hydrocarbon, then you
can be sure the products will be carbon dioxide and water. CO2 and H2O. That's it for combustion! See ya! .