Given the reaction: NH3(g)+O2(g)arrow NO(g)+H2O(g) What is the limiting reactant when there are .5 moles of O2 and 1.5 moles of NH3 available to react? How much excess is there? Choose matching definition Nh3, there is .5 moles of excess O2. O2, there is .moles of excess NH3. Nh3 there is 2 moles of excess Nh3. O2, there is 3 moles of excess O2.

Question

Given the reaction: NH3(g)+O2(g)arrow NO(g)+H2O(g) What is the limiting reactant when there are .5 moles of O2 and 1.5 moles of NH3 available to react? How much excess is there? Choose matching definition Nh3, there is .5 moles of excess O2. O2, there is .moles of excess NH3. Nh3 there is 2 moles of excess Nh3. O2, there is 3 moles of excess O2.

Answer 1

To determine the limiting reactant, we need to compare the mole ratio of the reactants with the stoichiometric ratio in the balanced chemical equation.The balanced chemical equation for the reaction is:

From the balanced equation, we can see that the stoichiometric ratio of

to

is 4:5.Now, let's compare the given amounts of

and

with the stoichiometric ratio:Given:

: 1.5 moles

: 0.5 molesTo find the limiting reactant, we need to calculate the amount of

required to completely react with 1.5 moles of

.Using the stoichiometric ratio, we can calculate the amount of

required as follows:

required =

=

= 1.875 molesSince we only have 0.5 moles of

available,

is the limiting reactant.To find the amount of excess

, we need to calculate the amount of

that remains after the reaction is complete.Using the stoichiometric ratio, we can calculate the amount of

that reacts with 0.5 moles of

as follows:

reacted =

=

= 0.4 molesThe amount of excess

is then:

excess =

initial -

reacted = 1.5 - 0.4 = 1.1 molesTherefore, the correct answer is:

, there is 1.1 moles of excess

.

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