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postnew [5]
2 years ago
10

What is the bond formation of N and H

Chemistry
2 answers:
Nimfa-mama [501]2 years ago
8 0
Hydrogen bonding between a water molecule and an ammonia (NH3) molecule. Note that the N atom in the NH3 molecule is attracted to H atom in the H20 molecule
Zielflug [23.3K]2 years ago
3 0

Answer:

A single bond, but it's also a hydrogen bond.

Explanation:

A hydrogen bond forms when hydrogen bonds to the 3 most electronegative atoms: Oxygen, Nitrogen, or Fluorine.

It's a single bond because hydrogen only has two valence electrons. Therefore, the rest of the electrons are placed around the nitrogen atom.

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• What type of rock is used for radiometric dating, Why?
sukhopar [10]
An igneous rock because its radiometric clock is reset, and potassiumargon measurements can be used to tell the number of years that have passed since metamorphism. <span />
3 0
3 years ago
The reaction below is at equilibrium. What would happen if more carbon were
schepotkina [342]

Explanation:

C_{(s)} + O_{2(g)} \rightleftharpoons CO_{2(g)}

<em>According to <u>le ch</u></em><em><u>-</u></em><em><u>atelier'</u></em><em><u>s</u></em><em><u> </u></em><em><u>principle</u> when a chemical reaction at equilibrium subjected to any stress, then the equilibrium shifts in that direction in which effect of stress is reduced.</em>

When we would add more number of carbon in above reaction then rate of forward reaction will increase to attain the equilibrium again.

\small \sf \: Thanks \:  for  \: joining  \: brainly \:  community!

5 0
2 years ago
The equilibrium constant for the reaction AgBr(s) Picture Ag+(aq) + Br− (aq) is the solubility product constant, Ksp = 7.7 × 10−
barxatty [35]

Answer:

The reaction will be  non spontaneous at these concentrations.

Explanation:

AgBr(s)\rightarrow Ag^+(aq) + Br^- (aq)

Expression for an equilibrium constant K_c:

K_c=\frac{[Ag^+][Br^-]}{[AgCl]}=\frac{[Ag^+][Br^-]}{1}=[Ag^+][Br^-]

Solubility product of the reaction:

K_{sp}=[Ag^+][Br^-]=K_c=7.7\times 10^{-13}

Reaction between Gibb's free energy and equilibrium constant if given as:

\Delta G^o=-2.303\times R\times T\times \log K_c

\Delta G^o=-2.303\times R\times T\times \log K_{sp}

\Delta G^o=-2.303\times 8.314 J/K mol\times 298 K\times \log[7.7\times 10^{-13}]

\Delta G^o=69,117.84 J/mol=69.117 kJ/mol

Gibb's free energy when concentration [Ag^+] = 1.0\times 10^{-2} M and [Br^-] = 1.0\times 10^{-3} M

Reaction quotient of an equilibrium = Q

Q=[Ag^+][Br^-]=1.0\times 10^{-2} M\times 1.0\times 10^{-3} M=1.0\times 10^{-5}

\Delta G=\Delta G^o+(2.303\times R\times T\times \log Q)

\Delta G=69.117 kJ/mol+(2.303\times 8.314 Joule/mol K\times 298 K\times \log[1.0\times 10^{-5}])

\Delta G=40.588 kJ/mol

  • For reaction to spontaneous reaction:  \Delta G.
  • For reaction to non spontaneous reaction:  \Delta G>0.

Since ,the value of Gibbs free energy is greater than zero which means reaction will be non spontaneous at these concentrations

5 0
3 years ago
What substance is oxidized in the following reaction? 4HCl + MnO2 → Cl2 + 2H2O + MnCl2
Blizzard [7]

Answer:

Cl⁻ was oxidized.

Explanation:

  • 4HCl + MnO₂ → Cl₂ + 2H₂O + MnCl₂

Oxidation can be defined as the process in which the oxidation number of a substance increases.

On the left side of the equation, Cl has a charge of -1 (in HCl); while on the right side of the equation Cl has a charge of 0 in Cl₂.

Thus, Cl⁻ was oxidized.

8 0
3 years ago
How many MOLECULES are in 50.0 grams of lithium phosphate?
Ray Of Light [21]
Answer: 2.60 x 10^23 molecules


50.0 grams x (1 mol/115.79 grams) = 0.431816219 moles

0.431816219 mol x (6.02 x 10^23 molecules/1 mol) = 2.599533638 x 10^23 molecules (final answer is rounded)
8 0
3 years ago
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