How did he get 15 moles?

What is the molarity of a 5.00 x 102 ml solution containing 2490 g of KI?

5.00*10^2ml = 500ml = .5L

KI has molar mass 166, so you have 15 moles of KI

15moles/.5L = 30moles/L = 30M

Given the reaction: Ni (s) + 4 CO (g)  Ni(CO)4 (g) E = –154 kJ, how many kilograms

of CO are required for this reaction to release 756 kJ of energy?

please

oops my bad. was gonna post new question, sorry i don't know the answer.

To understand how he got 15 moles, we need to look at the given information. We know that the solution contains 2490 grams of KI and we want to calculate the molarity of the solution.

First, we convert the volume of the solution from milliliters to liters. We are given that the volume is 5.00 x 10^2 mL. To convert mL to liters, we divide by 1000:

5.00 x 10^2 mL / 1000 = 0.5 L

So, the volume of the solution is 0.5 liters.

Next, we need to calculate the moles of KI in the solution. We know the molar mass of KI is 166 grams/mol. We can use the formula:

moles = mass / molar mass

moles = 2490 g / 166 g/mol = 15 moles

Therefore, there are 15 moles of KI in the solution.

To find the molarity of the solution, we use the formula:

molarity = moles of solute / volume of solution in liters

molarity = 15 moles / 0.5 L = 30 moles/L = 30 M

So, the molarity of the solution is 30 M.