what would the quantity of heat gained or lost be for 1.25 mol NaOH(s) dissolves in water?
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Dhsjie
To calculate the quantity of heat gained or lost when 1.25 mol of NaOH(s) dissolves in water, we need to use the molar enthalpy of dissolution, also known as the heat of solution.
The equation for the dissolution of NaOH(s) in water is:
NaOH(s) → Na+(aq) + OH-(aq)
The molar enthalpy of dissolution, denoted as ΔH diss, is the heat released or absorbed per mole of solute when it dissolves in a solvent.
According to experimental data, the molar enthalpy of dissolution of NaOH is approximately -44.5 kJ/mol.
To find the quantity of heat gained or lost, we use the equation:
Quantity of heat = number of moles × molar enthalpy of dissolution
Given that we have 1.25 mol of NaOH(s), we can calculate the quantity of heat gained or lost as follows:
Quantity of heat = 1.25 mol × (-44.5 kJ/mol)
Quantity of heat = -55.625 kJ
Therefore, the quantity of heat gained or lost when 1.25 mol of NaOH(s) dissolves in water is approximately -55.625 kJ. The negative sign indicates that heat is released during the dissolution process.
To determine the quantity of heat gained or lost when 1.25 mol of NaOH(s) dissolves in water, we need to calculate the enthalpy change of the dissolution process.
The enthalpy change (∆H) for dissolving a solid in a solvent is known as the enthalpy of solution. In this case, we need to find the enthalpy of solution for NaOH.
The enthalpy of solution can be calculated using the equation:
∆H = q / mol
Where:
∆H = enthalpy change (in J/mol)
q = heat gained or lost (in J)
mol = number of moles of the substance
To find the enthalpy of solution for NaOH, you will need to refer to a reliable reference source, such as a thermodynamic database or scientific literature. The enthalpy of solution for NaOH is -445.1 kJ/mol.
Now, we can calculate the quantity of heat gained or lost when 1.25 mol of NaOH(s) dissolves using the equation:
∆H = q / mol
Plugging in the values:
-445.1 kJ/mol = q / 1.25 mol
Rearranging the equation to solve for q:
q = -445.1 kJ/mol × 1.25 mol
q ≈ -556.375 kJ
Therefore, the quantity of heat gained or lost when 1.25 mol of NaOH(s) dissolves in water is approximately -556.375 kJ.