According to your investigation in part A, how do strong acids differ from weak acids? Select all the correct answers. Strong acids contain more A− than weak acids do. Strong acids contain more H3O+ than weak acids do. Strong acids contain more HA than weak acids do. Strong acids contain more OH− than weak acids do.

Strong acids contain more A− than weak acids do.

Strong acids contain more H3O+ than weak acids do

Explanation:

When we talk about a strong acid, we are referring to any acid that is completely dissociated or ionized when it is in an aqueous solution.

It is very eager to lose a proton, H+ in solution according Arrhenius definition.

In aqueous solution, a strong acid ionizes as follows:

HA(aq) + H2O → H3O+(aq) + A−(aq)

Since, strong acids ionize completely in solution, strong acids contain a greater H3O+ and A− concentration than solutions of weak acids.

Explanation:

The standard heat of formation is the enthalpy change for the formation of a compound from the elements at their standard states.

PCl₅ is formed by P and Cl, whose standard states are solid and diatomic gas.

You just must manipulate the two given equations to obtain an overall equation from P(s) and Cl₂(g).

Based of Hess' law, the enthalpy change of the overall equation is the algebraic sum of the individual equations.

If you multiply the first equation by 2 and reverse it you get:

Write the second equation:

Add them:

After computing:

Notice that the last calculation results in the standard enthalpy of formation for two moles of PCl₅(s). Thus, to obtain the enthalpy of formation per mol you must divide by 2:

Round to 3 signficant figures: -662kJ/mol