Question

The following thermochemical equation is for the reaction of sodium(s) with water(l) to form sodium hydroxide(aq) and hydrogen(g). 2Na(s) + 2H2O(l)2NaOH(aq) + H2(g) H = -369 kJ When 6.97 grams of sodium(s) react with excess water(l), kJ of energy are .
2) The following thermochemical equation is for the reaction of carbon monoxide(g) with water(l) to form carbon dioxide(g) and hydrogen(g).

CO(g) + H2O(l)Arrow.gif CO2(g) + H2(g) delta16-1.GIFH = 2.80 kJ

When 10.4 grams of carbon monoxide(g) react with excess water(l), kJ of energy are _________evolvedabsorbed.

Answer 1

Answer:

1) When 6.97 grams of sodium(s) react with excess water(l), 56.0 kJ of energy are evolved.

2) When 10.4 grams of carbon monoxide(g) react with excess water(l), 1.04 kJ of energy are absorbed.

Explanation:

1) The following thermochemical equation is for the reaction of sodium(s) with water(l) to form sodium hydroxide(aq) and hydrogen(g).

2 Na(s) + 2H₂O(l) ⇒ 2NaOH(aq) + H₂(g) ΔH = -369 kJ

The enthalpy of the reaction is negative, which means that 369 kJ of energy are evolved per 2 moles of sodium. The energy evolved for 6.97 g of Na (molar mass 22.98 g/mol) is:

$6.97g.\frac{1mol}{22.98g} .\frac{-369kJ}{2mol} =-56.0kJ$

2) The following thermochemical equation is for the reaction of carbon monoxide(g) with water(l) to form carbon dioxide(g) and hydrogen(g).

CO(g) + H₂O(l) ⇒ CO₂(g) + H₂(g)  ΔH = 2.80 kJ

The enthalpy of the reaction is positive, which means that 2.80 kJ of energy are absorbed per mole of carbon monoxide. The energy evolved for 10.4 g of CO (molar mass 28.01 g/mol) is:

$10.4g.\frac{1mol}{28.01g} .\frac{2.80kJ}{mol} =1.04kJ$