Suppose 1.65 moles of C6H6 react with excess oxygen gas to produce carbon dioxide and water. a. How many moles of carbon dioxide will be produced in this reaction?
b. How many moles of water will be produced in this reaction?
c. How many moles of oxygen gas will be consumed during the reaction?

they both have a y in them

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

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