HOW MANY MOLES OF SILVER IODIDE COULD BE PRODUCED IF THIS REACTION WAS STARTED WITH 4.3 MOL IODINE AND AN EXCESS OF SILVER?

Write and balance the equation.

Using the coefficients in the balanced equation, convert mols I2 to mols AgI
Now convert mols AgI to grams AgI. grams AgI = mols AgI x molar mass AgI.

To determine the number of moles of silver iodide that can be produced, we need to use the balanced chemical equation for the reaction and the stoichiometry of the reaction.

The balanced chemical equation for the reaction between iodine (I2) and silver (Ag) to form silver iodide (AgI) is:

2 Ag + I2 → 2 AgI

From the equation, we can see that for every 1 mole of iodine (I2), 2 moles of silver iodide (AgI) are produced.

Given that we have 4.3 moles of iodine (I2) and an excess of silver (Ag), we can assume that all the iodine (I2) will react completely.

To find the moles of silver iodide (AgI) produced, we can set up a ratio using the stoichiometry of the reaction:

(4.3 mol I2) x (2 mol AgI/1 mol I2) = 8.6 mol AgI

Therefore, if the reaction is started with 4.3 moles of iodine and an excess of silver, it can produce 8.6 moles of silver iodide.