Answer:
Both have the same amount of particles.
Explanation:
From Avogadro's hypothesis, we understood that 1 mole of any substance contains 6.02×10²³ particles.
This implies that 1 mole of Hydrogen contains 6.02×10²³ particles. Also, 1 mole of oxygen contains 6.02×10²³ particles.
Thus, 1 mole of Hydrogen and 1 mole of oxygen contains the same number of particles.
1) balance the equation
N2 + 3 H2 → 2 NH3
2) change the given grams to moles
(42.5 g N2) / (28.01344 g N2/mol) = 1.5171 mol N2
(10.1 g H2) / (2.015894 g H2/mol) = 5.0102 mol H2
3) compare moles * remember to multiply by the coefficient of the balanced equation
1.5171 moles of N2 would react completely with 1.5171 x (3/1) = 4.5513 moles of H2, but there is more H2 present than that, so H2 is in excess and N2 is the limiting reactant.
4) from the balanced equation moles of limiting reactant to moles produced and then multiply by MW of product
(1.5171 mol N2) x (2 mol NH3 / 1 mol N2) x (17.03056 g NH3/mol) = 51.7 g NH3
5) finally subtract the moles of limiting reactant from moles of excess reactant and multiply by excess reactants MW.
((5.0102 mol H2 initially) - (4.5513 mol H2 reacted)) x (2.015894 g H2/mol) =
0.925 g H2 left over
Answer and Explanation:
In Chemistry, the quantity or amount of a pure substance is given by:
- <em>mass</em><em> (in grams)</em>
- <em>Volume </em><em>(in millilitres or litres)</em>
- <em>Moles </em><em>(mol) </em>
Inter-conversion of units is allowed based on defined units and constituent of the substance.
I believe this explanation would be helpful and easy to follow.