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Oxana [17]
2 years ago
5

5.1169 mol of Ne is held at 0.9148 atm and 911 K. What is the volume of its container in liters?

Chemistry
1 answer:
sveticcg [70]2 years ago
5 0

By applying the Boyle's equation and substituting our given data the volume of the container was found to be 418.14 Litres

<h3>Boyle's  Law</h3>

Given Data

  • number of moles of Ne = 5.1169 mol
  • Pressure = 0.9148 atm
  • Temperature = 911 K

We know that the relationship between pressure and temperature is given as

PV = nRT

R = 0.08206

Making the volume subject of formula we have

V= nRT/P

Substituting our given data to find the volume we have

V = 5.1169*0.08206*911/0.9148

V = 382.522353554/0.9148

V = 418.14 L

Learn more about Boyle's law here:

brainly.com/question/469270

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olga nikolaevna [1]

Answer:

            Option-A is the correct answer

Explanation:

Lithium belong to group 1 metals. Hence, it can loose one electron to form lithium ion i.e. Li⁺¹ or Li⁺

While, Nitrogen is non-metal and hence has the ability to gain the electron lost by lithium metal. Furthermore, Nitrogen can gain maximum 3 electrons to acheive noble gas configuration. Hence, three Li atoms will loose their electrons and Nitrogen will gain those three electrons to form nitride ion i.e. N³⁻.

4 0
2 years ago
When iron rusts in air iron3 oxide is produced. How many moles of oxygen react with 28.0 mol of iron in the rusting reaction 4fe
Marrrta [24]
This the balanced equation based on the question 4Fe + 3O_2  -\ \textgreater \ 2Fe_2O_3.

We then proceed with the following calculations

28.0molFe*(\frac {3molO_2}{4mol Fe})= 21molO_2

The answer is 21molO_2 is produced.
5 0
3 years ago
What is required in order to melt a network solid?
mina [271]

Answer: In order to melt a network solid, a relatively large amount of heat is needed, sufficient to break the covalent bonds that hold the entire solid together

hope this helps

3 0
3 years ago
Using the following standard reduction potentials, Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Ni2+(aq) + 2 e- → Ni(s) E° = -0.23 V ca
lina2011 [118]

<u>Answer:</u> The above reaction is non-spontaneous.

<u>Explanation:</u>

For the given chemical reaction:

Ni^{2+}(aq.)+2Fe^{2+}(aq.)\rightarrow 2Fe^{3+}(aq.)+Ni(s)

Here, nickel is getting reduced because it is gaining electrons and iron is getting oxidized because it is loosing electrons.

We know that:

E^o_{(Fe^{3+}/Fe^{2+})}=0.77V\\E^o_{(Ni^{2+}/Ni)}=-0.23V

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the E^o_{cell} of the reaction, we use the equation:

E^o_{cell}=E^o_{cathode}-E^o_{anode}

E^o_{cell}=-0.23-0.77=-1.0V

Relationship between standard Gibbs free energy and standard electrode potential follows:

\Delta G^o=-nFE^o_{cell}

As, the standard electrode potential of the cell is coming out to be negative for the above cell. Thus, the standard Gibbs free energy change of the reaction will become positive making the reaction non-spontaneous.

Hence, the above reaction is non-spontaneous.

3 0
3 years ago
Scientists believe that interactions between atoms depend mostly on the arrangement of the outermost electrons in each atom. Thi
vova2212 [387]
I’m pretty sure it’s in a group (column) of the period table. Hope this helps :)))
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2 years ago
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