what is the magnitude of delta for [Ti(H2O)6]3+ in kj/mol?
delta what?
To determine the magnitude of Δ for [Ti(H2O)6]3+ in kJ/mol (kJ per mole), we need to refer to relevant thermodynamic data, specifically the standard enthalpy of formation (∆Hf) for the compound.
First, find the chemical equation representing the formation of [Ti(H2O)6]3+ (s) from its constituent elements in their standard states. The equation is as follows:
Ti3+ (aq) + 6 H2O (l) → [Ti(H2O)6]3+ (s)
Next, search for the standard enthalpy of formation (∆Hf) values for the reactants and products in the equation. Typically, these values are given per mole of the compound in kJ/mol.
Once you have the ∆Hf values for the reactants and product, you can calculate the enthalpy change (∆) for the reaction using the following formula:
∆ = ∑(∆Hf products) - ∑(∆Hf reactants)
Finally, substitute the given values into the formula, sum the ∆Hf values for the reactants and products, and calculate the Δ. The magnitude of Δ will provide the answer to the question.