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Sedbober [7]
3 years ago
13

Count the number of each type of atom in the equation below, and then balance the equation. Write In the numbers of atoms and co

efficient. Add a 1 if there should be no coefficient.
CS2(I)+O2(g)-CO2(g)+SO2(g)

__C __ S __ - __C __S __O



__ CS2(I)+ __ O2(g)- __ CO2(g)+__ SO2(g)
​
Chemistry
2 answers:
Galina-37 [17]3 years ago
8 0

1,2,2,1,1,4 is the numbers for the first equation

Studentka2010 [4]3 years ago
4 0

Answer:

Balanced equation

CS2(l) + 3O2(g)------> CO2(g) + 2SO2(g)

Explanation:

For a chemical equation to be balanced, the number of atoms of each element on the left Hans side of the reaction equation must equal the number of atoms of that element on the right hand side of the reaction equation.

Atoms of oxygen are six on both sides of the reaction equation. Atoms of sulphur are two while there is only one atom of carbon on both sides of the reaction equation.

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In a chemical reaction how does the mass of the reactants compare with the mass of the products?
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Answer:

The mass of the reactants compared with the mass of the products should be the same if the reactants are in stoichiometric amounts.

Explanation:

In this question, they ask about chemical reactions and the comparison of the mass of reactants and products. Firstly, it is necessary to introduce the mass conservation principle.

Mass conservation principle mentions that in a chemical reaction, the total mass of reactants is equal to the total mass of products (if the reaction is fully developed). It means mass is not created or destroyed, only transforms from reactants to products.

For example, the mass of sodium plus the mass of chlorine that reactswith the sodium equals the mass of the product sodium chloride.Because atoms are only rearranged in a chemical reaction, there mustbe the same number of sodium atoms and chlorine atoms in both thereactants and products.

Finally, we can conclude that The mass of the reactants compared with the mass of the products should be the same if the reactants are in stoichiometric amounts. 

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How is a coefficient used to balance an equation
ludmilkaskok [199]

Let's start to understand this question by a simple combustion reaction involving oxidation of Ethane in the presence of Oxygen. When Ethane is burned in the presence of Oxygen it produces Carbon Dioxide and Water respectively. Therefore, the equation is as,

                                C₂H₆  +  O₂    →    CO₂  +  H₂O

Above reaction shows the reaction and the equation is unbalanced. Balancing chemical equation is important because according to law of conservation of mass, mass can neither be created nor destroyed. Hence, we should balance the number of elements on both side.

                                       LHS                      RHS

Carbon Atoms                  2                            1

Hydrogen Atoms              6                           2

Oxygen Atoms                  2                           3

It means this equation is not obeying the law. Now, how to balance? One way is as follow,

                                C₂H₆  +  O₃    →    C₂O₂  +  H₆O

                                       LHS                      RHS

Carbon Atoms                  2                            2

Hydrogen Atoms              6                           6

Oxygen Atoms                  3                           3

We have balanced the equation by changing the subscripts. But, we have messed up the chemical composition of compounds and molecules like Oxygen is converted into Ozone.

Therefore, we will change the coefficients (moles) to balance the equation as,

                                C₂H₆  +  7/2 O₂    →    2 CO₂  +  3 H₂O

                                       LHS                      RHS

Carbon Atoms                  2                            2

Hydrogen Atoms              6                           6

Oxygen Atoms                  7                           7

Now, by changing the coefficients we have balanced the equation without disturbing the chemical composition of compounds and molecules.

3 0
3 years ago
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