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?

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

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.