Stoichiometry And Stoichiometric Calculations

Answer (d) 32

or According to question, of is converted into moles of moles moles of moles of Thus, total number of moles present originally was of of moles

The reaction between and is as follows: ### Step 1: Find the Molar Mass of The molar mass of is: ### Step 2: Find the Moles of Given that 10 g of is used and it is 90% pure, the effective mass of is: Now, calculate the moles of : ### Step 3: Moles of From the balanced equation, 1 mole of produces 1 mole of . Therefore, the moles of produced are also 0.09 mol. ### Step 4: Find the Mass of The molar mass of is: Thus, the mass of is: So, the mass of produced is approximately . Thus, the correct answer is: