Question

A 55.31 g sample of chlorine gas reacts with an excess of KI. What volume of iodine would be produced if the barometric pressure was 1.02 atm and the temperature was 25°C?

a) 0.45 L
b) 0.56 L
c) 0.62 L
d) 0.71 L

Answer 1

The volume of iodine produced is approximately 0.62 L

Step-by-step explanation:

To find the volume of iodine produced, we need to use the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

First, we need to convert the mass of chlorine gas to moles:

55.31 g Cl₂ x (1 mol Cl₂ / 70.90 g Cl₂) = 0.779 mol Cl₂

Next, we can use the balanced chemical equation to determine the mole ratio between Cl₂ and I₂:

1 mol Cl₂ : 1 mol I₂

So, 0.779 mol Cl₂ will react to produce 0.779 mol I₂

Now, we can use the ideal gas law to find the volume of iodine:

V = (nRT) / P

V = (0.779 mol)(0.0821 L/mol·K)(298 K) / 1.02 atm = 0.615 L

Therefore, the volume of iodine produced is approximately 0.62 L.