The Equator is where the doldrums are found.
Question:
Zinc metal is added to hydrochloric acid to generate hydrogen gas and is collected over a liquid whose vapor pressure is the same as pure water at 20.0 degrees C (18 torr). The volume of the mixture is 1.7 L and its total pressure is 0.987 atm. Determine the number of moles of hydrogen gas present in the sample.
A. 0.272 mol
B. 0.04 mol
C. 0.997 mol
D. 0.139 mol
E. 0.0681 mol
Answer:
The correct option is;
E. 0.0681 mol
Explanation:
The equation for the reaction is
Zn + HCl = H₂ + ZnCl₂
Vapor pressure of the liquid = 18 torr = 2399.803 Pa
Total pressure of gas mixture H₂ + liquid vapor = 0.987 atm
= 100007.775 Pa
Therefore, by Avogadro's law, pressure of the hydrogen gas is given by the following equation
Pressure of H₂ = 100007.775 Pa - 2399.803 Pa = 97607.972 Pa
Volume of H₂ = 1.7 L = 0.0017 m³
Temperature = 20 °C = 293.15 K
Therefore,

Therefore, the number of moles of hydrogen gas present in the sample is n ≈ 0.0681 moles.
The correct answer is that the energy will be transferred
into the system and as well as the solubility of lithium chloride will likely
increase. It Is because LiCl is soluble when is dispersed in hot water that is
why the solubility of lithium chloride will increase and that the heating
solution will likely transfer the heat energy in the system in which the energy
will be transferred in the system is correct.
<u>Answer:</u> The value of equilibrium constant is 0.997
<u>Explanation:</u>
We are given:
Percent degree of dissociation = 39 %
Degree of dissociation,
= 0.39
Concentration of
, c = 
The given chemical equation follows:

<u>Initial:</u> c -
<u>At Eqllm:</u>

So, equilibrium concentration of ![N_2O_4=c-c\alpha =[1-(1\times 0.39)]=0.61M](https://tex.z-dn.net/?f=N_2O_4%3Dc-c%5Calpha%20%3D%5B1-%281%5Ctimes%200.39%29%5D%3D0.61M)
Equilibrium concentration of ![NO_2=2c\alpha =[2\times 1\times 0.39]=0.78M](https://tex.z-dn.net/?f=NO_2%3D2c%5Calpha%20%3D%5B2%5Ctimes%201%5Ctimes%200.39%5D%3D0.78M)
The expression of
for above equation follows:
![K_{c}=\frac{[NO_2]^2}{[N_2O_4]}](https://tex.z-dn.net/?f=K_%7Bc%7D%3D%5Cfrac%7B%5BNO_2%5D%5E2%7D%7B%5BN_2O_4%5D%7D)
Putting values in above equation, we get:

Hence, the value of equilibrium constant is 0.997
Answer:
Explanation:
Given data:
Mass of N₂ = 48.7 g
Moles of N₂ = ?
Molecules of N₂ = ?
Mass of N₂O = ?
Moles of N₂O = ?
Atoms of N₂O = ?
Solution:
Chemical equation:
2N₂ + O₂ → 2N₂O
Number of moles of N₂:
Number of moles = mass/ molar mass
Number of moles = 48.7 g / 28 g/mol
Number of moles = 1.74 mol
Number of molecules of N₂:
1 mole = 6.022 × 10²³ molecules
1.74 mol× 6.022 × 10²³ molecules/1 mol
10.5 × 10²³ molecules
Now we will compare the moles of N₂ with N₂O from balance chemical equation:
N₂ : N₂O
2 : 2
1.74 : 1.74
Moles of N₂O:
1.74 mol
Mass of N₂O:
Mass = number of moles × molar mass
Mass = 1.74 mol × 44 g/mol
Mass = 76.56 g