Answer:
BaCl2 + 2AgNO3 ⇒ 2AgCl + Ba(NO3)2
Theoretical yield: 11.74g AgCl
Percent yield: 74.27%
Explanation:
BaCl2 + 2AgNO3 ⇒ 2AgCl + Ba(NO3)2
The percent yield = actual yield/ theoretical yield * 100%
Actual yield: The amount of product actually obtained from a reaction, in this case is 8.72g AgCl
Theoretical yield: The amount of product that would result if all the limiting reagent reacted. Now, we have the amount of BaCl2, so BaCl2 is our limiting reagent, because the maximum amount of product formed depends on how much of this reactant was present. Taking into consideration the balanced reaction, we can calculate the theoretical yield, so.
mass molar BaCl2 = 208.23 g/mol
mass molar AgCl = 143.32 g/mol
First,
moles of BaCl2= 8.53 g BaCl2*( 1mol BaCl2/ 208.23g BaCl2) = 0.04096mol
so, we have 0.04096 mol BaCl2, given that one mol of BaCl2 reacts to produce 2 mol of AgCl (watch the balanced reaction above) , so, the moles of AgCl are twice the moles of BaCl2, we should get 0.0819 mol AgCl and 11.74 g AgCl
g AgCl= 0.0819mol AgCl* (143.32g AgCl/ 1mol AgCl) = 11.74g AgCl theoretical yield
% yield = 8.72 g AgCl/ 11.74g AgCl* 100= 74.27%
Answer: The element expected to be most electronegative is Ca.
The element expected to be least electronegative is K.
Explanation:
Electronegativity is defined as the property of an element to attract a shared pair of electron towards itself.
Down the group:
The size of an atom increases as we move down the group because a new shell is added and electron gets added up.
As, the size of an element increases, the valence electrons gets away from the nucleus. So, the attraction between the nucleus and the shared pair of electrons decreases
Hence, electronegativity decreases moving from top to bottom down a group
Across a period:
The size of an atom decreases as we move across the period because the electrons get added to the same shell and the nuclear charge keeps on increasing. Thus the electrons get more tightly held by the nucleus.
As, the size of an element decreases, the valence electrons come near to the nucleus. So, the attraction between the nucleus and the shared pair of electrons increases.
Hence, electronegativity increases moving across left to right in a period.
Thus as K, Sc and Ca are arranged across a period, the electronegativity order is K< Sc < Ca.
Answer:
Ok so, b. A redox reaction occurs in an electrochemical cell, where silver (Ag) is oxidized and nickel (Ni) is reduced - In voltaic cells, also called galvanic cells, oxidation occurs at the anode and reduction occurs at the cathode. A mnemonic for this is "An Ox. Red Cat." So since silver is oxidized, the silver half-cell is the anode. And the nickel half-cell is the cathode...
i. Write the half-reactions for this reaction, indicating the oxidation half-reaction and the reduction half-reaction- The substance having highest positive  potential will always get reduced and will undergo reduction reaction. Here, zinc will always undergo reduction reaction will get reduced
ii. Which metal is the anode, and which is the cathode?-The anode is where the oxidation reaction takes place. In other words, this is where the metal loses electrons. The cathode is where the reduction reaction takes place.
iii. Calculate the standard potential (voltage) of the cell
Look up the reduction potential,
E
⁰
red
, for the reduction half-reaction in a table of reduction potentials
Look up the reduction potential for the reverse of the oxidation half-reaction and reverse the sign to obtain the oxidation potential. For the oxidation half-reaction,
E
⁰
ox
=
-
E
⁰
red
.
iv. What kind of electrochemical cell is this? Explain your answer.
All parts in the electrochemical cells are labeled in second figure. Following are the part in electrochemical cells
1) Anode 2) Cathode 3) gold Stripe (Electrode) 4) Aluminium Glasses (Electrode) 5) Connecting wires 6) Battery
Explanation:
Answer:
They are solid, have luster, are ductile, are malleable, brittle, make good semiconductors, conduct heat and electricity, have boiling points & melting points, have densities.
Answer:
2H2O2 --> O2 + 2H2O
It is decomposition of hydrogen peroxide into oxygen.
It can also be described a reaction showing how H2O2 acts as a reducing agent
H2O2(aq) ---------> O2(g) + 2H^+ (aq) + 2e E = + 1.77 V
2h2 O2 2h2o