If 25 grams of HNCO react, how many grams of CO2 are formed?

25.570 g

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