Concept explainers
When 9.59 g of a certain vanadium oxide is heated in the presence of hydrogen, and a new oxide of vanadium are formed. This new vanadium oxide has a mass of 8.76 g. When the second vanadium oxide undergoes additional heating in the presence Of hydrogen, 5.38 g of vanadium metal forms,
a. Determine the empirical formulas for the two vanadium oxides.
b. Write balanced equations for the Steps of the reaction.
c. Determine the mass of hydrogen needed to complete the steps of this reaction.
a)
Interpretation : The empirical formulas of the two-vanadium oxides need to be determined.
Concept introduction : Mass of elements reacts with each other to form compounds in a definite proportion.
Answer to Problem 109A
First vanadium oxide is V2O5 and other is VO2.
Explanation of Solution
Let assume first vanadium oxide,
VwOx and other is VyOz
V is 5.38 g and it is remaining constant throughout the reactions
For VwOx
Mass of oxygen = mass of vanadium oxide − mass of vanadium
= 9.59-5.38
= 4.21
Vanadium and oxygen form vanadium oxide in simple ratio
Simple ration vanadium to oxygen
So empirical formula of this VwOx is V2O5.
For VyOz
Mass of oxygen = mass of vanadium oxide − mass of vanadium
= 8.76-5.38
= 3.38
Vanadium and oxygen form vanadium oxide in simple ratio
Simple ration vanadium to oxygen
So empirical formula of this VyOz is VO2.
b)
Interpretation:
The balanced chemical equation for each step needs to be written.
Concept introduction:
A chemical reaction is said to be balanced, if there are equal number of atoms of same elements present in the reaction.
Answer to Problem 109A
Explanation of Solution
The balanced chemical equations will be as follows:
From the above equations, in first reaction 1 mol of
1 mol of
c)
Interpretation:
The mass of hydrogen needed to complete both steps of reaction needs to be determined.
Concept introduction:
The relation between mass and molar mass is as follows:
Here, m is mass and M is molar mass.
Answer to Problem 109A
0.5324 g of hydrogen
Explanation of Solution
So, 0.0530 moles of hydrogen is require for first reaction
So, 2 times the 0.1056 that is 0.2112 moles of hydrogen is required for second reaction
Total moles of hydrogen = 0.0530 + 0.2112 = 0.2642
Molar mass of hydrogen = 2.0158 g/mol
Mass of hydrogen =
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Glencoe Chemistry: Matter and Change, Student Edition
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