Question

"The following reaction shows sodium carbonate reacting with calcium hydroxide.

Na2CO3 + Ca(OH)2 + 2NaOH + CaCO3
How many grams of NaOH are produced from 20.0 grams of Na2CO3?
(Molar mass of Na = 22.989 g/mol, C = 12.01 g/mol, O = 15.999 g/mol, Ca = 40.078
g/mol, H = 1.008 g/mol)
1) 12.2 grams
2) 15.1 grams
3) 24.4 grams
4) 30.2 grams

Answer 1

To determine the grams of NaOH produced from 20.0 grams of Na2CO3, we need to use the balanced equation and calculate the mole ratio between Na2CO3 and NaOH.

Step-by-step explanation:

To determine the grams of NaOH produced from 20.0 grams of Na2CO3, we need to use the balanced equation and calculate the mole ratio between Na2CO3 and NaOH. The balanced equation is:

Na2CO3 + Ca(OH)2 → 2NaOH + CaCO3

The molar mass of Na2CO3 is 22.99 g/mol + 2 x 12.01 g/mol + 3 x 15.999 g/mol = 105.99 g/mol.

Using the molar mass and the given mass of Na2CO3, we can calculate the number of moles of Na2CO3: 20.0 g / 105.99 g/mol = 0.188 mol.

Since the mole ratio between Na2CO3 and NaOH is 1:2, the number of moles of NaOH produced is 2 x 0.188 mol = 0.376 mol.

Finally, we can calculate the grams of NaOH produced using the molar mass of NaOH: 0.376 mol x 22.989 g/mol = 8.64 grams (rounded to one decimal place).