Solid sodium hydroxide reacts with gaseous carbon dioxide to form solid sodium carbonate salt and liquid water. Formulate the balanced chemical reaction When 1.85 mol NaOH and 1.00 mol carbon dioxide heat, how many moles of sodium carbonate can be theoretically produced? How many moles of the excess starting material remains?

Question

Gustavo

Chemistry

5 May, 11:40

Solid sodium hydroxide reacts with gaseous carbon dioxide to form solid sodium carbonate salt and liquid water. Formulate the balanced chemical reaction When 1.85 mol NaOH and 1.00 mol carbon dioxide heat, how many moles of sodium carbonate can be theoretically produced? How many moles of the excess starting material remains?

+4

Answers (1)

Know the Answer?

Tucker Coleman · Answer 1

a) 0.925 mol Na2CO3 can be theoretically produced

b) 0.075 moles of the excess starting material remains

Explanation:

balaced chemical:

2 NaOH (s) + CO2 (g) ↔ Na2CO3 (s) + H2O (aq)

1.85n 1.00n Xn

moles theor. Na2CO3:

⇒ nNaCO3 = 1.85nNaOH * (nNa2CO3 / 2nNaOH)

⇒ nNa2CO3 = 0.925nNa2CO3

moles of the excess:

⇒moles CO2 react = 1.85nNaOH * nCO2 / 2nNaOH = 0.925n CO2

⇒moles CO2 excess = 1.00n - 0.925n = 0.075n excess CO2