Question

SnO2 is reduced by carbon according to this reaction: SnO2 + C ???? Sn + CO2. How many liters of CO2 are produced if 300.0 grams of tin are produced at STP? How many grams of SnO2 are required to produce 1800.0 grams of tin? How much tin is produced per 100.0 grams of carbon used?

Answer 1

Explanation:

The given reaction is as follows.

         $SnO_{2} + C \rightarrow Sn + O_{2}$

a).   Molar mass of $SnO_{2}$ is [(mass of Sn) + (2 × mass of O)].

Therefore, molar mass of $SnO_{2}$ = (118.7 + 2 × 16) g/mol = 150.7 g/mol

Since, it is known that number of moles equal mass divided by molar mass. So, moles of Sn will be calculated as follows.

               No. of moles = $\frac{mass}{molar mass of SnO_{2}}$

                                      = $\frac{300 g}{150.7 g/mol}$

                                      = 2.53 mol

As it is given that 1 mole of $SnO_{2}$ produces 1 moles of Sn and 1 moles of $CO_{2}$. Hence, 2.53 moles of $SnO_{2}$ will also produce 2.53 moles of Sn and 2.53 moles of $CO_{2}$.

Volume of 1 mole of $CO_{2}$ at STP is 22.4 L. Therefore, volume of 2.53 moles of $CO_{2}$ will be calculated as follows.

                  2.53 × 22.5 L = 56.67 L

Hence, 56.67 L of $CO_{2}$ are produced if 300.0 grams of tin are produced at STP.

b).  Mass of tin is given as 1800.0 g. So, number of moles will be calculated as follows.

               No. of moles = $\frac{mass}{molar mass of tin}$

                                      = $\frac{1800.0 g}{118.7 g/mol}$

                                      = 15.2 moles

As 15.2 moles of $SnO_{2}$ produces 15.2 moles of Sn. Therefore, weight of $SnO_{2}$ will be calculated as follows.

                   Mass = no. of moles × molar mass of $SnO_{2}$

                             = 15.2 moles × 150.7 g/mol

                             = 2290.64 g

Hence, 2290.64 grams of $SnO_{2}$ are required to produce 1800.0 grams of tin.

c).   Mass of carbon given is 100.0 grams.

             No. of moles = $\frac{mass}{molar mass of carbon}$

                                    = $\frac{100 g}{12 g/mol}$

                                      = 8.33 moles

As, 1 mole of carbon is produced by 1 mole of tin. So, 8.33 mole of carbon will be produced by 8.33 moles of tin.

Therefore, calculate mass of tin produced as follows.

                        Mass = no. of moles × molar mass of Sn

                             = 8.33 moles × 118.7 g/mol

                             = 988.8 g

Hence, 988.8 grams of tin will be produced per 100 grams of carbon used.