Answer:
25.570 g
Step-by-step explanation:
Assuming the chemical reaction in question;
4HNCO + 6NO → 5N₂ + 2H₂O + 4CO₂
We are given;
Mass HNCO as 25 grams
We are required to calculate the mass of CO₂ formed
Step 1: Number of moles of HNCO
To calculate the number of moles we divide mass by the molar mass
Number of moles = Mass ÷ molar mass
Molar mass of HNCO = 43.03 g/mol
Therefore,
Moles of HNCO = 25 g ÷ 43.03 g/mol
= 0.581 moles
Step 2: Moles of CO₂ formed
From the equation 4 moles of HNCO reacts to produce 4 moles of CO₂
Therefore, the mole ratio of HNCO to CO₂ is 1 : 1
Thus, moles of CO₂ is equal to moles of HNCO
Moles of CO₂ = 0.581 moles
Step 3: Mass of CO₂
Mass is calculated by multiplying number of moles by molar mass
Molar mass of CO₂ is 44.01 g/mol
Therefore;
Mass = 0.581 moles × 44.01 g/mol
= 25.570 g
Therefore, the mass of CO₂ formed is 25.570 g