Consider preparing ammonia gas by the following reaction: N2(g) + 3H2(g)
===>
2NH3(g)
If you have 28.02 g of N2 and excess H2, how many grams of NH3(g) can be produced.
6.06 g
14.01 g
34.08 g
68.16 g
28.02 g

34.08 g

Explanation:

Take the atomic mass of N=14.0, H=1.0/

no. of moles=mmass/molar mass

no. of moles of N2 used = 28.02 / (14x2)

=1.0007mol

From the equation, the mole ratio of N2 : NH3 = 1: 2,

so one mole of N2 produces 2 moles of NH3.

Using this ratio, we can deduce that the no. of moles of NH3 = 1.0007x2

= 2.001428mol

mass = no. of moles x molar mass

Hence,

mass of NH3 produced = 2.001428 x (14+1x3)

= 34.03

≈C

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.