Question

2KI(aq) + Cl2(g) → 2KCl(aq) + I2(g) How many moles of I2 are produced? mol How many moles of Cl2 are used? mol How many grams of Cl2 (g) are used? grams

Answer 1

The question requires calculating the moles of I2 and Cl2, and the mass of Cl2 used, given their balanced chemical reaction. Without the initial quantity of either reactant, these values cannot be determined.

Step-by-step explanation:

The question pertains to a chemical reaction in which iodine (I2) is produced from the reaction of potassium iodide (KI) and chlorine gas (Cl2). From the provided information, we need to find:

• The number of moles of I2 produced
• The number of moles of Cl2 used
• The mass of Cl2 used in grams

However, to calculate these, we need a starting quantity for either KI or Cl2. Since that information is not provided, we cannot proceed with the computation. If the amount of either reactant is known, we can use the stoichiometric coefficients from the balanced equation to find the answers. Typically, to find the number of moles of a substance, we would use the molar mass as a conversion factor. For example, the molar mass of Cl2 is 70.90 g/mol which is used to convert grams to moles.

Answer 2

All depends on how much of product we use but imagine we use 1mol of KI

there's a 2:1 ratio of KI to I₂ so 1/2 = 0.5mol of I₂

the same applied to the Cl₂ there is a 2:1 ratio, therefore, 0.5mol of Cl₂ is required

to find mass (g) multiple moles by RFM = 0.5 x 71 = 35.5g

Hope that helps :)