Problemas
4NH_(3)+5O_(2)-gt 4NO+6H_(2)O How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 0.37g 0.045 1.35g 11.19
Roztwór
Gabriel
élite · Tutor durante 8 años
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Respuesta
To determine how many grams of NO are formed when 6.30g of ammonia react with 1.80g of oxygen, we need to follow these steps:1. Calculate the molar masses of the reactants and products.2. Convert the masses of the reactants to moles.3. Determine the limiting reactant.4. Use stoichiometry to find the mass of NO produced.### Step 1: Calculate Molar Masses-
:
g/mol-
:
g/mol-
:
g/mol### Step 2: Convert Masses to Moles- Moles of
:
- Moles of
:
### Step 3: Determine the Limiting ReactantThe balanced equation is:
From the stoichiometry of the reaction:- 4 moles of
react with 5 moles of
.- Therefore, 1 mole of
reacts with
moles of
.Calculate the required moles of
for the given moles of
:
Since we only have 0.05625 moles of
,
is the limiting reactant.### Step 4: Use Stoichiometry to Find the Mass of NO ProducedUsing the limiting reactant (
):- According to the balanced equation, 5 moles of
produce 4 moles of
.- Therefore, 0.05625 moles of
will produce:
Now, convert the moles of
to grams:
Therefore, the mass of NO formed is
.The correct answer is: