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:
# of protons: 17
Mass #: 36
#of electrons: 17
Element: Chlorine (Cl)
Explanation:
# of protons: based on atomic#
Mass #: protons+neutrons
#of electrons: based on atomic# if it's neutral charge
Element: use the Periodic Table to find element 17 (each element has their corresponding atomic#)
Answer:
12.6 g
Explanation:
Step 1: Write the balanced decomposition reaction
2 Fe₂O₃ ⇒ 4 Fe + 3 O₂
Step 2: Calculate the moles corresponding to 18.0 g of Fe₂O₃
The molar mass of Fe₂O₃ is 159.69 g/mol.
18.0 g × 1 mol/159.69 g = 0.113 mol
Step 3: Calculate the moles of Fe formed from 0.113 moles of Fe₂O₃
The molar ratio of Fe₂O₃ to Fe is 2:4. The moles of Fe formed are 4/2 × 0.113 mol = 0.226 mol
Step 4: Calculate the mass corresponding to 0.226 moles of Fe
The molar mass of Fe is 55.85 g/mol.
0.226 mol × 55.85 g/mol = 12.6 g
True. The CAUSE of any magnetic field is not understood by anyone.
The diagram is a simple circuit of a battery connected to a light bulb in a circuit with a switch.
The corresponding names, starting with the battery and going counterclockwise, are:
1) Battery
2) Wire
3) socket
4) switch