10*=? There is not enough information for me to solve, but you can use this formula to solve.
mass(1.00x10*kg) / molar mass of (NH4)2SO4 x molar mass of NH3
How many kilograms of NH3 are needed to produce 1.00×10*kg of (NH4)2SO4?
2 answers
Almost but not quite there.
First, I assume that * meant a typo and the question was for 1.00E8 kg (NH4)2SO4.
So 1E8 kg x (2*molar mass NH3)/molar mass (NH4)2SO4
That 2 is necessary because there are two NH3 molecules in (NH4)2SO4. Or to put it another way, the equation for the formation of (NH4)2SO4 is
H2SO4 + 2NH3 ==> (NH4)2SO4
The chemical factor which Ryan and I used above is now "old fashioned" and is not taught in chemistry classes today. Instead they do this.
mols (NH4)2SO4 = grams/molar mass = ?
Now convert mols (NH4)2SO4 to mols NH3. That's 2* mols (NH4)2SO4.
Now convert mols NH3 to grams NH3. grams = mols x molar mass.
But note how much faster the use of a chemical factor is than the "new & improved" way.
First, I assume that * meant a typo and the question was for 1.00E8 kg (NH4)2SO4.
So 1E8 kg x (2*molar mass NH3)/molar mass (NH4)2SO4
That 2 is necessary because there are two NH3 molecules in (NH4)2SO4. Or to put it another way, the equation for the formation of (NH4)2SO4 is
H2SO4 + 2NH3 ==> (NH4)2SO4
The chemical factor which Ryan and I used above is now "old fashioned" and is not taught in chemistry classes today. Instead they do this.
mols (NH4)2SO4 = grams/molar mass = ?
Now convert mols (NH4)2SO4 to mols NH3. That's 2* mols (NH4)2SO4.
Now convert mols NH3 to grams NH3. grams = mols x molar mass.
But note how much faster the use of a chemical factor is than the "new & improved" way.
1 answer