Answer:
23.2 mols
Explanation:
(23.2 mol H2)(2 mol H2O) /(2 mol H2) = 23.2 mol H2O
you have to do stoichiometry - so start of with what you are given, which is 23.2 mols of hydrogen, then to cancel out mols of hydrogen, divide by what is in the equation: so 23.2 mols H2 / 2 mols H2. Next, to get mols of H2O multiply that number by the mols of water in the equation.
this answer makes sense because as you can see in the equation, there are 2 H2:2 H2O, so the amounts should be the same.
hope this helps! make sure to practice because it is ESSENTIAL that you understand this, especially if you plan on taking ap chem. good luck! :)
Answer:
B, C
Explanation:
The atoms or ions with the valid Lewis dot structures are B and C.
In A;
The Lewis structure of the carbon is correct. Each of the four dots represent the four valence electrons.
The nitrogen with one dot on top, left and to the bottom and has a charge of minus 3 is wrong. For it to have a charge of -3 it must have 8 lewis dots ( two on the top, right, bottom and to the left)
The nitrogen with four dots (on top, right, bottom and to the left) is wrong.
In B;
An oxygen has two dots on top and bottom and one dot to the left and to the right. This is correct , the 6 dots represent the valence electrons of oxygen.
In C;
A carbon has two dots on top, right, bottom and to the left and a charge of plus four. This is correct because the charge indicates that it has gained four extra electrons so its valence electrons is now 8.
In D;
An oxygen has two dots on top, left and to the bottom and a charge of minus 2. This is wrong because the lewis dots are incomplete. Two dots are missing.
B,c and f are true,but I doubt about g cause I don't know anything about electron's dimention
Answer:
4.61 x 10ˉ⁴ mole H₂(g)
Explanation:
Given electric current for 2 min. => 12.4ml of wet H₂(g) at 25⁰C & 715Torr => ? moles H₂(g)
PV = nRT => n = PV/RT
• P = P(H₂) + P(H₂O) = 715Torr = 715mm = P(H₂) + 23.8mm
=> P(H₂) = (715 – 23.8)mm = 619.2mm = 619.2mm/760mm/Atm = 0.815Atm
• V = 12.8ml = 0.0128L
• R = 0.08206 L∙Atm/mol∙K
• T = 25⁰C = 298K
Substituting … n = PV/RT
=> n = (0.815Atm)(0.0128L)/(0.08206 L∙Atm/mol∙K)(298K) = 4.61 x 10ˉ⁴ mole H₂(g)
Molar mass F₂O₃ = 159.69 g/mol
1 mole ------------------ 159.69 g
0.7891 moles ---------- ? g
mass = 0.7891 x 159.69 / 1
= 126.01 g
hope this helps!
