In order to solve this, we need to know the standard cell potentials of the half reaction from the given overall reaction.
The half reactions with their standard cell potentials are:
<span>2ClO−3(aq) + 12H+(aq) + 10e- = Cl2(g) + 6H2O(l)
</span><span>E = +1.47
</span>
<span>Br(l) + 2e- = 2Br-
</span><span>E = +1.065
</span>
We solve for the standard emf by subtracting the standard emf of the oxidation from the reducation, so:
1.47 - 1.065 = 0.405 V
Answer:
4KO₂ + 2CO₂ -> 2K₂CO₃ + 3O₂
<u> Step 1: Find the moles of O₂.</u>
n(O₂) = mass/ Mr.
n(O₂) = 100 / 32 = 3.125 mol
<u>Step 2: Find the ratio between KO₂ and O₂.</u>
<u>KO₂ </u> : <u> O₂</u>
4 : 3
4/3 : 1
(4*3125)/3 : 3.125
=4.167 mol of KO₂
Thus now we know, to produce 100 g of O₂, we need 4.167mol of KO₂
<u>Step 3: Find the mass of KO₂:</u>
<u />
mass = mol * Mr. (KO₂)
Mass = 4.167* 71.1
Mass = 296.25 g
Answer:
1) phosphorus and chlorine
type of bond = polar covalent
They share their electrons and due to difference in electronegativities the form polar covalent bond.
2) potassium and oxygen
type of bond = ionic
Due to high difference in electronegativities the form ionic bond.
3) fluorine and fluorine
type of bond = non polar covalent
They share their electrons and due to same electronegativities the form non polar covalent bond.
4) copper and aluminum
type of bond = metallic
copper and aluminum make metallic bond like other metals and mostly helpful in making alloys.
5) carbon and fluorine
type of bond = polar covalent
They share their electrons and due to difference in electronegativities the form polar covalent bond.
6) carbon and hydrogen
type of bond = polar covalent
They share their electrons and due to difference in electronegativities the form polar covalent bond.
7) aluminum and oxygen
type of bond = ionic
Due to high difference in electronegativities the form ionic bond.
8) silver and copper
type of bond = metallic
silver and copper make metallic bond like other metals and mostly helpful in making alloys.
Answer:
Copper-63
Explanation:
Since atomic masses are averages of a certain element's mass from all of its isotopes, the average of the atomic mass will be closest to the most abundant isotope. Knowing that the mass of copper-63 is 63 amu and the average atomic mass of copper is 63.546, its most abundant isotope must be copper-63
