Based on the nature of chemical equilibrium, the system reached equilibrium first at the time T2.
<h3>What is chemical equilibrium?</h3>
Chemical equilibrium refers to the state of a reversible chemical reaction in which the rate of forward reaction for the the formation is equal to the rate of backward reaction for the formation of reactants.
In the table of the decomposition reaction given above, the system reached equilibrium first at the time T2 when the concentration of the reactant and products were the same.
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From other sources, the given mass of the solute that is being dissolved here is 7.15 g Na2CO3 - 10H2O. We use this amount to convert it to moles of Na2CO3 by converting it to moles using the molar mass then relating the ratio of the unhydrated salt with the number of water molecules. And by the dissociation of the unhydrated salt in the solution, we can calculate the moles of Na+ ions that are present in the solution.
Na2CO3 = 2Na+ + CO3^2-
7.15 g Na2CO3 - 10H2O (1 mol / 402.9319 g) (1 mol Na2CO3 / 1 mol Na2CO3 - 10H2O) ( 1 mol Na2CO3 / 1 mol Na2CO3-10H2O ) ( 2 mol Na+ / 1 mol Na2CO3) = 0.04 mol Na+ ions present
The net ionic equation is written as H^+(aq) + OH^-(aq) -------> H2O(l)
<h3>What is the net ionic equation?</h3>
The term net ionic equation refers to the equation that shows the ions that underwent a change in the reaction. We have to note that the reaction species here must be ionic species which are able to dissociate into ions in solutions.
Now the first step is to put down the molecular equation. The molecular equation shows the reaction of the compounds as follows;
HCI (aq) + NaOH (ag)-> NaCI (aq) +H2O(l)
Next, we put own the complete ionic reaction equation as follows;
H^+(aq) + Cl^-(aq) + Na^+(aq) + OH^-(aq) -------> Na^+(aq) + + Cl^-(aq) + H2O(l)
Next we have the net ionic equation;
H^+(aq) + OH^-(aq) -------> H2O(l)
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