Concept explainers
Interpretation: The mass of ammonia required to react with excess of oxygen to produce same amount of water as prepared from reacting
Concept introduction: The ratio of mass of substance to its molar mass is said to be number of moles of that substance.
The ratio of amount of any two compounds involved in a
Answer to Problem 28A
The mass of ammonia required to react with excess of oxygen to produce same amount of water as prepared from reacting
Explanation of Solution
The complete balanced equation for the reaction between methane and oxygen to produce carbon dioxide and water is:
The number of moles of reactants,
The molar mass of
Putting the values:
From the balanced reaction, the mole ratio between water and methane is 2:1 that is 2 moles of water are produced from 1 mole of methane. So, the number of moles of water produced from
Now, the balanced reaction between ammonia and oxygen to produce nitrogen monoxide and water is:
From the balanced reaction, the mole ratio between water and ammonia is 6:4 that is 6 moles of water are produced from 4 moles of ammonia. So, the number of moles of ammonia required to produce
The mass of ammonia is calculated using formula:
The molar mass of
Hence, the mass of ammonia required to react with excess of oxygen to produce same amount of water as prepared from reacting
Chapter 9 Solutions
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