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4 years ago

In water, HNO3 produces H+ ions. Which is the name for HNO3 in an aqueous solution?

2 answers:

ozzi4 years ago

7 0

Nitric acid is the chemical name for HNO3(aq). The compound is composed of hydrogen, nitrogen and oxygen.

Alborosie4 years ago

4 0

Answer: It is named as nitric acid in aqueous solution.

Explanation:

$HNO_3$ is an acid because it releases hydrogen ions when dissolved in water. The chemical equation for the ionization of $HNO_3$ follows:

$HNO_3(aq.)\rightarrow H^+(aq.)+NO_3^-(aq.)$

When an element is present in the higher oxidation state in a compound, a suffix '-ic' is added at the end.

When an element is present in the lowest oxidation state in a compound, a suffix '-ous' is added at the end.

Nitrogen shows oxidation state of +5 and +3. In the given compound, nitrogen is present in +5 oxidation state. Thus, in the naming of the compound, a suffix '-ic' is added.

Hence, the given compound is named as nitric acid in aqueous solution.

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What is the thermal energy needed to completely melt 9.60 mol of ice at 0.0 C

inysia [295]

The thermal energy needed to completely melt 9.60 mole of ice at 0.0 C is 57.8 Kj

Explanation
ice melt to form water

The molar heat of fusion for water is 6.02 Kj/mol
Thermal energy = moles x molar heat of fussion for water

=9.6 mol x6.02 kj/mol =57.8 Kj

4 0

3 years ago

Read 2 more answers

If 8.50 g of phosphorus reacts with hydrogen gas at 2.00 atm in a 10.0-L container at 298 K, calculate the moles of PH3 produced

ahrayia [7]

Answer:

The moles of PH₃ produced are 0.2742 and the total number of moles of gas present at the end of the reaction is 0.6809.

Explanation:

Phosphorus reacts with H₂ according to the balanced equation:

P₄ (s) + 6 H₂ (g) ⇒ 4 PH₃ (g)

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:

P₄: 1 mole
H₂: 6 moles
PH₃:4 moles

Being the molar mass of the compounds:

P₄: 124 g/mole
H₂: 2 g/mole
PH₃: 34 g/mole

The following mass amounts of each compound participate in the reaction:

P₄: 1 mole* 124 g/mole= 124 g
H₂: 6 mole* 2 g/mole= 12 g
PH₃: 4 moles* 34 g/mole= 136 g

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P * V = n * R * T

In this case you know:

P= 2 atm
V= 10 L
n= ?
R= 0.082 $\frac{atm*L}{mol*K}$
T= 298 K

Replacing:

2 atm*10 L= n*0.082 $\frac{atm*L}{mol*K}$ *298 K

and solving you get:

$n=\frac{2 atm*10 L}{0.082\frac{atm*L}{mol*K}*298 K }$

n=0.818 moles

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

To determine the limiting reagent, you can use a simple rule of three as follows: if 6 moles of H₂ react with 124 g of P₄, 0.818 moles of H₂ with how much mass of P₄ will it react?

$mass of P_{4}=\frac{0.818 moles of H_{2}*124 grams of P_{4}}{6 moles of H_{2}}$

mass of P₄= 16.90 grams

But 16.90 grams of P₄ are not available, 8.50 grams are available. Since you have less mass than you need to react with 0.818 moles of H₂, phosphorus P₄ will be the limiting reagent.

Then you can apply the following rules of three:

If 124 grams of P₄ produce 4 moles of PH₃, 8.50 grams of P₄, how many moles do they produce?

$moles of PH_{3} =\frac{8.5 grams of P_{4}*4 moles of PH_{3} }{124grams of P_{4}}$

moles of PH₃=0.2742

If 124 grams of P₄ react with 6 moles of H₂, 8.50 grams of P₄ with how many moles of H₂ do they react?

$moles of H_{2} =\frac{8.5 grams of P_{4}*6 moles of H_{2} }{124grams of P_{4}}$

moles of H₂= 0.4113

If you have 0.818 moles of H₂, the number of moles of gas H₂ present at the end of the reaction is calculated as:

0.818 - 0.4113= 0.4067

Then the total number of moles of gas present at the end of the reaction will be the sum of the moles of PH₃ gas and H₂ gas that did not react:

0.2742 + 0.4067= 0.6809

Finally, the moles of PH₃ produced are 0.2742 and the total number of moles of gas present at the end of the reaction is 0.6809.

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3 years ago

When performing labratory experiments, which of the following items is ALWAYS necessary to use?

densk [106]

All of the the answers are are correct but a fume hood is more for if you are dealing with chemicals that can produce fumes the are deadly to people

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4 years ago

Which is not a compound?Electrons spin in shells around the nucleus. The closest shell (n = 1) can contain a maximum of _____ el

melisa1 [442]

The closest shell (n = 1) can contain a maximum of 2 electrons.

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4 years ago

Write the balanced electrochemical reaction for when zinc reacts with a copper solution. Label what is being oxidized and what i

Fed [463]

The balanced equation would be $Zn + Cu^{2+} ---- > Cu + Zn^{2+}$

<h3>Electrochemical equations</h3>

Zn reacts with Cu solution according to the following equation:

$Zn + Cu^{2+} ---- > Cu + Zn^{2+}$

In the reaction, $Cu^{2+}$ is reduced according to the following: $Cu^{2+} + 2 e^- -- > Cu$

While Zn is oxidized according to the following: $Zn - 2e^- --- > Zn^{2+}$

Thus, giving the overall equation of; $Zn + Cu^{2+} ---- > Cu + Zn^{2+}$

More oxidation-reduction equations can be found here: brainly.com/question/13699873

#SPJ1

5 0

2 years ago