Question

From the following balanced equation, 4 NH,(g) +50,() — 4 NO(g) + 6H,O(1) how many grams of NO can be formed from 3.78 g 0,? Select the correct answer below: O 2.55 g O 2.84 g O 4.43 g O 5.04 g

Answer 1

From the balanced equation, 4 moles of NO is formed from 5 moles of O2.

So, 4/5 moles of No is formed from 1 mole of O2.

Number of moles of O2 = mass/molar mass

The molar mass of O2 = 2* atomic mass of O2 = 2*16 = 32 g

So, number of moles of O2 = 3.78/32 = 0.118

So, number of moles of NO produced = 0.118*4/5 = 0.0945

Mass of NO produced = number of moles * molar mass

Molar mass of NO = atomic mass of Nitrogen + atomic mass of O = 14+16 = 30g

So, Mass of No produced = 0.0945*30 = 2.835 g