Determine if the following reaction is spontaneous under standard conditions.

Zn(s) + 4 CN¡V(aq) + Ag2CrO4(s) „³ Zn(CN)42¡V(aq) + 2 Ag(s) + CrO42¡V(aq)

The symbols are garbled.

To determine if the given reaction is spontaneous under standard conditions, we need to look at the standard Gibbs free energy change (ΔG°) of the reaction.

The standard Gibbs free energy change can be calculated using the equation:

ΔG° = ΣG°(products) - ΣG°(reactants)

Where ΣG°(products) is the sum of the standard Gibbs free energy of the products, and ΣG°(reactants) is the sum of the standard Gibbs free energy of the reactants.

First, let's determine the standard Gibbs free energy of each species involved in the reaction using a reliable source or a Gibbs free energy table.

ΔG° for Zn(CN)42-(aq) can be determined based on the concentration of Zn^2+ and CN^- ions (which are typically given in tables). Similarly, the ΔG° for CrO42-(aq) can be determined based on the concentration of CrO42- ions.

Next, we need to determine the ΔG° values for Ag(s), Zn(s), and Ag2CrO4(s). These values are zero because pure solids and pure metals are considered to have no free energy change in their standard states.

Now, sum up the standard Gibbs free energy of the products and reactants based on the coefficients in the balanced chemical equation.

ΣG°(products) = ΔG° of Zn(CN)42-(aq) + ΔG° of Ag(s) + ΔG° of CrO42-(aq)
ΣG°(reactants) = ΔG° of Zn(s) + 4 * ΔG° of CN-(aq) + ΔG° of Ag2CrO4(s)

Finally, substitute the values into the equation for ΔG°:

ΔG° = ΣG°(products) - ΣG°(reactants)

If the calculated ΔG° is negative, then the reaction is spontaneous under standard conditions. If ΔG° is positive or zero, then the reaction is not spontaneous under standard conditions.

Please note that the specific values for ΔG° need to be obtained from a reliable source or reference table, as they may vary depending on temperature and other factors.