CHEMISTRY MIDDLE SCHOOL

A closed container is filled with 2 moles of hydrogen gas and 2 moles of oxygen gas. The gases react to form water.Write a balanced equation for this reaction.

Answers

Answer 1
Answer:

Answer:

2H_2+O_2=2H_2O

Explanation:

The chemical formula for hydrogen is H while chemical formula for oxygen is O

Considering that two moles of hydrogen and 2 moles of oxygen react to form water, the equation will be

2H_2+2O_2=H_2O

The number of oxygen molecules don't balance on both LHS and RHS hence to balance it, we put it as follows

2H_2+O_2=2H_2O

Normally, two moles of hydrogen require only one mole of oxygen to form two moles of water.

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Answers

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#11.) When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 77.4 mol of iron in the rusting reaction?4Fe(s) + 3O2(g) → 2Fe2O3(s)

Select one:
a. 58
b. 100
c. 77
d. 120

#13.) For the reaction CH4 + 2O2 → CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 161.0 g of methane?

Select one:
a. 10.03
b. 20.06
c. 2584
d. 3.351

Answers

Answer 1)Option A) 58.05


In the given reaction of iron forming rust when reacts with the oxygen.


4 Fe_((s)) + 3O_(2)_((g) ----> 2Fe_(2)O_(3)_((s))


We can clearly see that, 4 moles of iron reacts with 3 moles of oxygen to give 2 moles of iron oxide.


So 4 Fe : 3 O and 77.4 moles of Fe : x moles of O


(3 X 77.4) / 4 = 58.05


So when we solve we get x as 58.05.


Hence the no. of moles of oxygen will be 58.


Answer 2) Option A) 10.03


The number of moles of carbon dioxide produced when 161.0 g of methane undergoes combustion will be 10.03


as we know the molar mass of methane is 16.043g


As we can see in the reaction the mole ratio is 1:1;


1 mole of methane produces 1 mole of carbondioxide.


So, 161 g / 16.043 g = 10.03 moles of Carbon dioxide.

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Answers

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Potential energy is energy at rest. 

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Answers

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Answers

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Answers

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