Answer:
47.47 g of CO₂ is the amount formed.
Explanation:
The reaction is:
2C₆H₅COOH(aq) + 15O₂(g) → 14CO₂(g) + 6H₂O(l)
Let's apply the formula for the percent yield
Percent yield of reaction = (Produced yield/Theoretical yield) . 100
First of all we convert the moles of CO₂ to mass: 1.30 mol . 44 g /1 mol = 57.2 g. So now, we replace:
(Produced yield / 57.2 g ). 100 = 83
Produced yield / 57.2 g = 83 / 100
Produced yield / 57.2 g = 0.83
Produced yield = 0.83 . 57.2g → 47.47 g of CO₂
Answer:
2H2 + O2 -----> 2H2O
Not sure about the second question though.
Answer:
Explanation:
a ) period 4 noble gas is krypton
isoelectronic with it are Sr ⁺² and Br⁻
compound is SrBr₂
b ) Period 3 noble gas is Argon
isoelectronic with it are Mg⁺² and O⁻²
compound is MgO
c) 2+ ion is the smallest with a filled d subshell is Zn⁺² , smallest halogen
is F⁻
compound is ZnF₂
d ) ions from the largest and smallest ionizable atoms in Period 2
Li⁺ and F⁻
compound is LiF
Answer: (2)3.0 mol
Explanation: 222.3g= 222.3/74= 3.0 mol
1mol Ca(OH)2 is 74g
