Question

When Na(s) reacts with H₂O(1) to form NaOH(aq) and H₂(g), 184 kJ of energy are evolved for each mole of Na(s) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank.

Answer 1

A balanced thermochemical equation for the reaction of sodium with water includes smallest integer coefficients and the energy term on the products side indicating an exothermic process. The equation is 2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g) -184 kJ.

Step-by-step explanation:

The student is asking for help with writing a thermochemical equation for the reaction of solid sodium (Na) with liquid water (H₂O) to form aqueous sodium hydroxide (NaOH) and hydrogen gas (H₂). The enthalpy change of the reaction is given as 184 kJ per mole of Na reacted and is exothermic.

The balanced thermochemical equation for this reaction should incorporate the smallest integer coefficients possible for each substance and include the energy term on the appropriate side of the equation. Since 184 kJ of energy are evolved, indicating that it is released, the energy term should be placed on the products side of the equation with a negative sign, which denotes an exothermic process.

The balanced thermochemical equation for the reaction would be:

2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g) + -184 kJ