2. Calculate the number of grams of nitrogen dioxide that are produced from 4 moles of nitric oxide.
2NO(g) + O2(g)  2NO2(g)

mass of nitrogen dioxide = 368g

Explanation:

From the equation:

2 moles of NO = 2 moles of 2 NO2

4 moles of NO = x moles of NO2

x = (2 × 4)/2 = 8/2 = 4 moles of NO2

No. of moles = reacting mass/ molecular weight

Reacting mass = No. of moles × molecular weight

Reacting mass = 4 × 92 = 368g

i believe the answer is a.

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.