Br2 + 2LiF → 2LiBr + F2 Given: If 3.6 moles of Br2, react with 9.4 moles of LiF
a) How many moles of F, are produced? I​

Br2 + 2LiF → 2LiBr + F2

Given: If 3.6 moles of Br2, react with 9.4 moles of LiF

a) How many moles of F, are produced? I

Explanation:

How many moles of F, are produced? I

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa