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hram777 [196]
3 years ago
9

26. A Grignard's reagent may be made by

Chemistry
1 answer:
Marat540 [252]3 years ago
8 0
Its pretty easy, correct answer is D
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Name the type of bond between atoms in ammonia molecule. Give a reason for your answer
Likurg_2 [28]

Answer:

Covalent bonds are formed when electrons are shared between elements that are nonmetals. The ammonium ion, NH+4 , would have covalent bonds because both nitrogen and hydrogen are nonmetals. ... The rest of the bonds all contain electrons from both hydrogen and nitrogen, so they would be considered ordinary covalent bonds.

6 0
3 years ago
Read 2 more answers
What’s the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of nitrogen, and 1 mo
satela [25.4K]

Answer:

p

(

CO

2

)

=

0.58

atm

Explanation:

p

(

CO

2

)

=

Total pressure

⋅

Mole fraction of CO

2

=

1.05

⋅

5

5

+

3

+

1

=

1.05 ⋅ 5/9 = 0.58 atm

Explanation:

7 0
3 years ago
Which of the following is an example of potential energy?
marishachu [46]
Answer: d
explanation:
7 0
3 years ago
A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). W
Agata [3.3K]

Answer : The 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

Explanation :

Galvanic cell : It is defined as a device which is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy. It is also known as the voltaic cell or electrochemical cell.

In the galvanic cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

We are taking the value of standard reduction potential form the standard table.

E^0_{[Ag^{+}/Ag]}=+0.80V

E^0_{[Cu^{2+}/Cu]}=+0.34V

In this cell, the component that has lower standard reduction potential gets oxidized and that is added to the anode electrode. The second forms the cathode electrode.

The balanced two-half reactions will be,

Oxidation half reaction (Anode) : Cu(s)\rightarrow Cu^{2+}(aq)+2e^-

Reduction half reaction (Cathode) : Ag^{+}(aq)+e^-\rightarrow Ag(s)

Thus the overall reaction will be,

Cu(s)+2Ag^{+}(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)

From this we conclude that, 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

Hence, the 'Ag' is produced at the cathode electrode and 'Cu' is produced at anode electrode under standard conditions.

7 0
3 years ago
Do step 3 as outlined in the lab guide. Record your results in the appropriate blanks.
PolarNik [594]

Explanation:

Do the step 3 as outlined in the lab guide. record your results in the appropriate blank.

D

8 0
3 years ago
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