Nitrogen dioxide (NO2) is a toxic gas produced by cars and factories. If a car produces one mole of NO2 during a 10 mile drive, how many grams of nitrogen dioxide are produced?

Explanation:

molecular weight of NO₂ is 14 + 2 x 16 = 46

So one mole of nitrogen dioxide will have mass of 46 grams .

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

the atomic mass is the bottom number on the element.

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