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3 years ago

If you begin with 72 grams of Nickel, how many moles of Ni would you have?

Chemistry

1 answer:

Marianna [84]3 years ago

6 0

Answer: 1.2 Moles of Nickel

Explanation:

So you have to transfer grams to moles.

You do this by dividing your beginning mass by the atomic mass of the element (found on the periodic table).

1 mole is equal to the atomic mass of the element. The atomic mass of Nickel is 58.6934 rounded to the proper significant figures will be 59.

72 Grams Nickel / 59 grams = 1.2 moles of Nickel

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Which of the following correctly represents the electronic distribution in the Si atom? A. 2,8,3 | B. 2,3,8 | C. 2,4,8 | D. 2,8,

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The electron distribution in the Si atom : D. 2,8,4

<h3>Further explanation</h3>

The maximum number of electrons that can be filled in the nth electron shell is 2n²(n=shell)

K shell (n = 1) maximum 2 x 1² = 2 electrons
L shell (n = 2) maximum 2 x 2² = 8 electrons
M shell (n = 3) maximum 2 x 3² = 18 electrons
N shell (n = 4) maximum 2 x 4² = 32 electrons

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K shell = 2

L shell = 8

M shell = 4

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3 years ago

Read 2 more answers

Write the full unabbreviated electrons configuration of the following elements

I am Lyosha [343]

Answer:

Explanation:

Sodium:

Na₁₁ = 1s² 2s² 2p⁶ 3s¹

Iron:

Fe₂₆= 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

Bromine:

Br₃₅ = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵

Barium:

Ba₅₆ = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s²

Cobalt:

Co₂₇ = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁷

Silver:

Ag₄₇ = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s¹ 4d¹⁰

Tellurium:

Te₅₂= 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁴

Radium:

Ra₈₈ = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s²

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4 years ago

A chemist designs a galvanic cell that uses these two half-reactions:

Nonamiya [84]

Answer :

(a) Reaction at anode (oxidation) : $4Fe^{2+}\rightarrow 4Fe^{3+}+4e^-$

(b) Reaction at cathode (reduction) : $O_2+4H^++4e^-\rightarrow 2H_2O$

(c) $O_2+4H^++4Fe^{2+}\rightarrow 2H_2O+4Fe^{3+}$

(d) Yes, we have have enough information to calculate the cell voltage under standard conditions.

Explanation :

The half reaction will be:

Reaction at anode (oxidation) : $Fe^{2+}\rightarrow Fe^{3+}+e^-$ $E^0_{anode}=+0.771V$

Reaction at cathode (reduction) : $O_2+4H^++4e^-\rightarrow 2H_2O$ $E^0_{cathode}=+1.23V$

To balance the electrons we are multiplying oxidation reaction by 4 and then adding both the reaction, we get:

Part (a):

Reaction at anode (oxidation) : $4Fe^{2+}\rightarrow 4Fe^{3+}+4e^-$ $E^0_{anode}=+0.771V$

Part (b):

Reaction at cathode (reduction) : $O_2+4H^++4e^-\rightarrow 2H_2O$ $E^0_{cathode}=+1.23V$

Part (c):

The balanced cell reaction will be,

$O_2+4H^++4Fe^{2+}\rightarrow 2H_2O+4Fe^{3+}$

Part (d):

Now we have to calculate the standard electrode potential of the cell.

$E^o=E^o_{cathode}-E^o_{anode}$

$E^o=(1.23V)-(0.771V)=+0.459V$

For a reaction to be spontaneous, the standard electrode potential must be positive.

So, we have have enough information to calculate the cell voltage under standard conditions.

4 0

3 years ago

If you begin with 72 grams of Nickel, how many moles of Ni would you have?​

If you begin with 72 grams of Nickel, how many moles of Ni would you have?