Solved problem
Electrolysis of aqueous NaCl gives the products shown below. Calculate the mass in grams of Cl2 that can be produced from 1.00 of 0.150 NaCl.
2NaCl(aq) + 2H2O
H2(g) + Cl2(g) + 2NaOH(g)
2NaCl(aq) + 2H2O
H2(g) + Cl2(g) + 2NaOH(g)Known | c(NaCl) V(NaCl) | n = c × V Step 1 | n(NaCl) |
Step 2 | n(Cl2) | m = n × M Step 3 | m(Cl2) | Unknown |
n(NaCl) = 0.150 mol
n(NaCl) = 0.150 mol
n(Cl2) = 0.0750 mol
m(Cl2) = 0.0750mol × 70.906 g mol–1
m(Cl2) = 5.325 g
n(NaCl) = 0.150 mol
| 0.150 mol | = | n(Cl2) |
| 2 | 1 |
m(Cl2) = 0.0750
m(Cl2) = 5.325 g
Step 1: Calculate the amount in moles of the known sustance from given information (mass of pure substance or volume and concentration of a solution).
Step 2: The amounts in moles of known and unknown are related through the balanced equation for the reaction.
Step 3: The mass is calculated from the calculated amount in moles and the known molar mass.
Step 2: The amounts in moles of known and unknown are related through the balanced equation for the reaction.
Step 3: The mass is calculated from the calculated amount in moles and the known molar mass.