How many molecules (not moles) of nh3 are produced from 8.95×10−4 g of h2?

 1.8 x 10²³molecules

Explanation:

Given parameters:

Mass of H₂ = 8.95 x 10⁻⁴g

Unknown:

Number of molecules of NH₃ = ?

The equation of the reaction: N₂ + 3H₂ ⇄ 2NH₃

To solve this problem:

           Number of moles of H₂ =

           Number of moles =

          Number of moles = 0.00045mol

          3 moles of H₂ produced 2 moles of NH₃

         0.00045mol of H₂ yields 0.000299mol of NH₃

To find the number of molecules of NH₃ produced, we use the expression below:

        Number of molecules = number of moles x 6.02 x 10²³

  Number of molecules of NH₃ = 0.000299 x 6.02 x 10²³ =

                                                                              1.8 x 10²³molecules

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.