2SO2 + O2 ==> 2SO3
moles of SO2 present = 98.6 g x 1 mole/64 g = 1.54 moles
moles O2 needed = 1/2 (1.54 moles) = 0.770 moles O2 needed(b/c mole ratio of O2:SO2 is 1:2)
Assuming the questioner is intending to produce SO2:
5.48/32.065=0.17 mol
Hence 0.17 x NA = 1.029x1023 molecules of O2 are needed.
SO3 is Molecular Weight 80. 40.0g is thus 0.5 moles so there are 3 x 0.5 x 6.022 x 1023 atoms of oxygen = 9.033 x 1023 oxygen atoms in 40.0 g of SO3.
1,8 of moles of O2 are required.
4.63x10^23
This is not a common reaction at standard temperature and pressure.
Yes, it is possible.
1 mol of H2 is necessary.
To form ammonia, reaction is N(2) + 3H(2) ---> 2NH(3) + H(2)O. As you can see for 1 mole of nitrogen three moles of hydrogen is required. Hence for your question, 1.13 moles nitrogen is required.
The coefficient (the number in front of the reactant) tells you the number of moles involved.
This is not a common reaction at standard temperature and pressure.
Do you mean this reaction? C6H12O6 + 6O2 -> 6CO2 + 6H2O 6 moles oxygen required. --------------------------------
1,5665 moles barium phosphate
I assume you mean this reaction. Zn + 2HCl --> ZnCl2 + H2 2.3 moles zinc (2 moles HCl/1 mole Zn) = 4.6 moles hydrochloric acid needed ========================
0.449 mol
Yes, it is possible.
2CO(g) + O2(g) → 2CO2(g)
1 mol of H2 is necessary.
They are called coefficients. They represent the number of moles of that element required for the reaction to be completed as written in relation to the number of moles for the other elements. They can also be considered the number of molecules required (different from moles), but most combustion reactions include 1/2 as a coefficient for O2. So don't get confused.
To form ammonia, reaction is N(2) + 3H(2) ---> 2NH(3) + H(2)O. As you can see for 1 mole of nitrogen three moles of hydrogen is required. Hence for your question, 1.13 moles nitrogen is required.
Mass-mass problems can be solved in various ways. You should start by writing a balanced equation for chemical reaction involved and eventually change the mass into moles which will facilitate the comparison and allow you to calculate the number of moles required.
The coefficient (the number in front of the reactant) tells you the number of moles involved.