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stiv31 [10]
3 years ago
14

What is the name of n2o4

Chemistry
2 answers:
quester [9]3 years ago
8 0

Answer:

Dinitrogen tetroxide, commonly referred to as nitrogen tetroxide (NTO), and occasionally (usually among ex-USSR/Russia rocket engineers) as amyl, is the chemical compound N2O4.

Gre4nikov [31]3 years ago
7 0
Dinitrogen Tetraoxide

Explanation:
Since nitrogen and oxygen are two non metals, they make up a binary covalent compound.

In N2O4, since there is two nitrogen’s, using the chart in the image below we can see that we would use the “di“ prefix (in this case). Since there are 4 oxygen’s we would add the prefix “tetra” as stated in the chart and turn oxygen into oxide; as the rule is add “ide” to the ending of a nonmetal in a binary covalent/ionic compound.

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Explain, in your own words, what volumic mass is
ira [324]

Answer:

The density (more precisely, the volumetric mass density; also known as specific mass), of a substance is its mass per unit volume. The symbol most often used for density is ρ (the lower case Greek letter rho), although the Latin letter D can also be used.

5 0
3 years ago
A student cleaned their glassware with tap water (known to contain chloride ions). They then attempted to make a 0.020 M solutio
Rina8888 [55]

Answer:

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Explanation:

The silver nitrate, AgNO₃, dissolves in water as follows:

AgNO₃(aq) → Ag⁺(aq) + NO₃⁻(aq)

The Ag⁺ reacts with Cl⁻ producing AgCl(s), a white insoluble salt. The net ionic equation that describes the formation of the precipitate is:

<h3>Ag⁺(aq) + Cl⁻(aq) → AgCl(s)</h3><h3 /><h3 />
4 0
3 years ago
What is the mass in grams of 5.50 mol of sodium?
Zolol [24]

Answer:

126.5g

Explanation:

n=<u>m</u><u> </u>

M

where n is moles

m is mass of substance

M is molar mass

molar mass of sodium is 23g/mol

m=nM

m=5.5(23)

m=126.5

8 0
3 years ago
Given the partial equation:
Nikolay [14]

Answer : The balanced chemical equation in acidic medium will be,

IO_3^-(aq)+2Sn^{2+}(aq)+6H^+(aq)\rightarrow I^-(aq)+2Sn^{4+}(aq)+3H_2O(l)

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Rules for the balanced chemical equation in acidic solution are :

First we have to write into the two half-reactions.

Now balance the main atoms in the reaction.

Now balance the hydrogen and oxygen atoms on both the sides of the reaction.

If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the less number of oxygen are present.

If the hydrogen atoms are not balanced on both the sides then adding hydrogen ion (H^+) at that side where the less number of hydrogen are present.

Now balance the charge.

The given chemical reaction is,

IO_3^-(aq)+Sn^{2+}(aq)\rightarrow I^-(aq)+Sn^{4+}(aq)

The oxidation-reduction half reaction will be :

Oxidation : Sn^{2+}\rightarrow Sn^{4+}

Reduction : IO_3^-\rightarrow I^-

First balance the main element in the reaction.

Oxidation : Sn^{2+}\rightarrow Sn^{4+}

Reduction : IO_3^-\rightarrow I^-

Now balance oxygen atom on both side.

Oxidation : Sn^{2+}\rightarrow Sn^{4+}

Reduction : IO_3^-\rightarrow I^-+3H_2O

Now balance hydrogen atom on both side.

Oxidation : Sn^{2+}\rightarrow Sn^{4+}

Reduction : IO_3^-+6H^+\rightarrow I^-+3H_2O

Now balance the charge.

Oxidation : Sn^{2+}\rightarrow Sn^{4+}+2e^-

Reduction : IO_3^-+6H^++4e^-\rightarrow I^-+3H_2O

The charges are not balanced on both side of the reaction. Thus, we are multiplying oxidation reaction by 2 and the adding both equation, we get the balanced redox reaction.

Oxidation : 2Sn^{2+}\rightarrow 2Sn^{4+}+4e^-

Reduction : IO_3^-+6H^++4e^-\rightarrow I^-+3H_2O

The balanced chemical equation in acidic medium will be,

IO_3^-(aq)+2Sn^{2+}(aq)+6H^+(aq)\rightarrow I^-(aq)+2Sn^{4+}(aq)+3H_2O(l)

5 0
3 years ago
What will the charge oxidiation state be for boron
artcher [175]

3+

So, compounds of boron contain boron in a positive oxidation state, generally +3. The sum of oxidation numbers of all constituent atoms of a given molecule or ion is equal to zero or the charge of the ion, respectively. ... In most of the stable compounds of boron, its oxidation number is +3

7 0
3 years ago
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