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Ganezh [65]
3 years ago
10

How many Grams of NO is produced if 12g of O2 is combined with excess ammonia?

Chemistry
1 answer:
stich3 [128]3 years ago
5 0

Answer:

9g

Explanation:

moles O2 = mass / Mr = 12 / 2(16.0) = 0.375

ratio O2 : NO = 5:4

moles NO produced = 0.375 * 4/5 = 0.3

mass NO = Mr * mol = (14.0+16.0) * 0.3 = 9g

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A container of hydrogen at 172 kPa was decreased to 85.0 kPa producing a new volume of 3L. What was the original volume?
Aneli [31]

Answer:

<h2>The answer is 1.48 L</h2>

Explanation:

In order to find the original volume we use the same for Boyle's law which is

P_1V_1 = P_2V_2

where

P1 is the initial pressure

P2 is the final pressure

V1 is the initial volume

V2 is the final volume

Since we are finding the original volume

V_1 =  \frac{P_2V_2}{P_1}  \\

From the question

P1 = 172 kPa = 172000 Pa

P2 = 85 kPa = 85000 Pa

V2 = 3 L

We have

V_1 =  \frac{85000 \times 3}{172000}  =  \frac{255000}{172000}  =  \frac{255}{172}  \\  = 1.482558139...

We have the final answer as

<h3>1.48 L</h3>

Hope this helps you

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3 years ago
How is the orbital configuration of neutral atoms related to the atoms chemical properties
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Answer:

Explanation:

Chemical properties of atoms relies solely on the number of electrons they contain, more particularly, the valence or outermost electrons in the orbit round the nucleus of an atom.

A neutral atom is one that has not gained or lost electron or even shared electrons with any other atom.

On close examination of how electrons are distributed in the orbits of an atom, we can know if an atom will gain or lose electrons in a reaction. This is very important in determining the chemical properties of an atom.

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Which of the following is an example of convection?
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Can some one tell me the best position in sex
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3 years ago
When the following aqueous solutions are mixed together, a precipitate forms. Balance the net ionic equation in standard form fo
rewona [7]

<u>Answer:</u>

<u>For (a):</u> The balanced net ionic equation is 2Ag^{+}(aq)+S^{2-}(aq)\rightarrow Ag_2S(s) and the sum of coefficients is 4

<u>For (b):</u> The balanced net ionic equation is Pb^{2+}(aq)+2Cl^{-}(aq)\rightarrow PbCl_2(s) and the sum of coefficients is 4

<u>For (c):</u> The balanced net ionic equation is Ca^{2+}(aq)+CO_3^{2-}(aq)\rightarrow CaCO_3(s) and the sum of coefficients is

<u>For (d):</u> The balanced net ionic equation is Ba^{2+}(aq)+2OH^{-}(aq)\rightarrow Ba(OH)_2(s) and the sum of coefficients is 4

<u>For (e):</u> The balanced net ionic equation is Ag^{+}(aq)+Cl^{-}(aq)\rightarrow AgCl(s) and the sum of coefficients is 3

<u>Explanation:</u>

Net ionic equation is defined as the equations in which spectator ions are not included.

Spectator ions are the ones that are present equally on the reactant and product sides. They do not participate in the reaction.

  • For (a): Sodium sulfide and silver nitrate

The balanced molecular equation is:

Na_2S(aq)+2AgNO_3(aq)\rightarrow 2NaNO_3(aq)+Ag_2S(s)

The complete ionic equation follows:

2Na^{+}(aq)+S^{2-}(aq)+2Ag^+(aq)+2NO_3^{-}(aq)\rightarrow 2Na^+(aq)+2NO_3^-(aq)+Ag_2S(s)

As sodium and nitrate ions are present on both sides of the reaction. Thus, they are considered spectator ions.

The net ionic equation follows:

2Ag^{+}(aq)+S^{2-}(aq)\rightarrow Ag_2S(s)

Sum of the coefficients = [2 + 1 + 1] = 4

  • For (b): Lead(II) nitrate and sodium chloride

The balanced molecular equation is:

2NaCl(aq)+Pb(NO_3)_2(aq)\rightarrow 2NaNO_3(aq)+PbCl_2(s)

The complete ionic equation follows:

2Na^{+}(aq)+2Cl^{-}(aq)+Pb^{2+}(aq)+2NO_3^{-}(aq)\rightarrow 2Na^+(aq)+2NO_3^-(aq)+PbCl_2(s)

As sodium and nitrate ions are present on both sides of the reaction. Thus, they are considered spectator ions.

The net ionic equation follows:

Pb^{2+}(aq)+2Cl^{-}(aq)\rightarrow PbCl_2(s)

Sum of the coefficients = [2 + 1 + 1] = 4

  • For (c): Calcium nitrate and potassium carbonate

The balanced molecular equation is:

K_2CO_3(aq)+Ca(NO_3)_2(aq)\rightarrow 2KNO_3(aq)+CaCO_3(s)

The complete ionic equation follows:

2K^{+}(aq)+CO_3^{2-}(aq)+Ca^{2+}(aq)+2NO_3^{-}(aq)\rightarrow 2K^+(aq)+2NO_3^-(aq)+CaCO_3(s)

As potassium and nitrate ions are present on both sides of the reaction. Thus, they are considered spectator ions.

The net ionic equation follows:

Ca^{2+}(aq)+CO_3^{2-}(aq)\rightarrow CaCO_3(s)

Sum of the coefficients = [1 + 1 + 1] = 3

  • For (d): Barium nitrate and sodium hydroxide

The balanced molecular equation is:

2NaOH(aq)+Ba(NO_3)_2(aq)\rightarrow 2NaNO_3(aq)+Ba(OH)_2(s)

The complete ionic equation follows:

2Na^{+}(aq)+2OH^{-}(aq)+Ba^{2+}(aq)+2NO_3^{-}(aq)\rightarrow 2Na^+(aq)+2NO_3^-(aq)+Ba(OH)_2(s)

As sodium and nitrate ions are present on both sides of the reaction. Thus, they are considered spectator ions

The net ionic equation follows:

Ba^{2+}(aq)+2OH^{-}(aq)\rightarrow Ba(OH)_2(s)

Sum of the coefficients = [2 + 1 + 1] = 4

  • For (e): Silver nitrate and sodium chloride

The balanced molecular equation is:

NaCl(aq)+AgNO_3(aq)\rightarrow NaNO_3(aq)+AgCl(s)

The complete ionic equation follows:

Na^{+}(aq)+Cl^{-}(aq)+Ag^{+}(aq)+NO_3^{-}(aq)\rightarrow Na^+(aq)+NO_3^-(aq)+AgCl(s)

As sodium and nitrate ions are present on both sides of the reaction. Thus, they are considered spectator ions.

The net ionic equation follows:

Ag^{+}(aq)+Cl^{-}(aq)\rightarrow AgCl(s)

Sum of the coefficients = [1 + 1 + 1] = 3

8 0
3 years ago
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