Answer:
Explanation:
Assume that you have mixed 135 mL of 0.0147 mol·L⁻¹ NiCl₂ with 190 mL of 0.250 mol·L⁻¹ NH₃.
1. Moles of Ni²⁺
2. Moles of NH₃
3. Initial concentrations after mixing
(a) Total volume
V = 135 mL + 190 mL = 325 mL
(b) [Ni²⁺]
(c) [NH₃]
3. Equilibrium concentration of Ni²⁺
The reaction will reach the same equilibrium whether it approaches from the right or left.
Assume the reaction goes to completion.
Ni²⁺ + 6NH₃ ⇌ Ni(NH₃)₆²⁺
I/mol·L⁻¹: 6.106×10⁻³ 0.1462 0
C/mol·L⁻¹: -6.106×10⁻³ 0.1462-6×6.106×10⁻³ 0
E/mol·L⁻¹: 0 0.1095 6.106×10⁻³
Then we approach equilibrium from the right.
Ni²⁺ + 6NH₃ ⇌ Ni(NH₃)₆²⁺
I/mol·L⁻¹: 0 0.1095 6.106×10⁻³
C/mol·L⁻¹: +x +6x -x
E/mol·L⁻¹: x 0.1095+6x 6.106×10⁻³-x
![K_{\text{f}} = \dfrac{\text{[Ni(NH$_{3}$)$_{6}^{2+}$]}}{\text{[Ni$^{2+}$]}\text{[NH$_{3}$]}^{6}} = 2.0 \times 10^{8}](https://tex.z-dn.net/?f=K_%7B%5Ctext%7Bf%7D%7D%20%3D%20%5Cdfrac%7B%5Ctext%7B%5BNi%28NH%24_%7B3%7D%24%29%24_%7B6%7D%5E%7B2%2B%7D%24%5D%7D%7D%7B%5Ctext%7B%5BNi%24%5E%7B2%2B%7D%24%5D%7D%5Ctext%7B%5BNH%24_%7B3%7D%24%5D%7D%5E%7B6%7D%7D%20%3D%202.0%20%5Ctimes%2010%5E%7B8%7D)
Kf is large, so x ≪ 6.106×10⁻³. Then
![K_{\text{f}} = \dfrac{\text{[Ni(NH$_{3}$)$_{6}^{2+}$]}}{\text{[Ni$^{2+}$]}\text{[NH$_{3}$]}^{6}} = 2.0 \times 10^{8}\\\\\dfrac{6.106 \times 10^{-3}}{x\times 0.1095^{6}} = 2.0 \times 10^{8}\\\\6.106 \times 10^{-3} = 2.0 \times 10^{8}\times 0.1095^{6}x= 345.1x\\x= \dfrac{6.106 \times 10^{-3}}{345.1} = 1.77 \times 10^{-5}\\\\\text{The concentration of Ni$^{2+}$ at equilibrium is $\large \boxed{\mathbf{1.77 \times 10^{-5}}\textbf{ mol/L}}$}](https://tex.z-dn.net/?f=K_%7B%5Ctext%7Bf%7D%7D%20%3D%20%5Cdfrac%7B%5Ctext%7B%5BNi%28NH%24_%7B3%7D%24%29%24_%7B6%7D%5E%7B2%2B%7D%24%5D%7D%7D%7B%5Ctext%7B%5BNi%24%5E%7B2%2B%7D%24%5D%7D%5Ctext%7B%5BNH%24_%7B3%7D%24%5D%7D%5E%7B6%7D%7D%20%3D%202.0%20%5Ctimes%2010%5E%7B8%7D%5C%5C%5C%5C%5Cdfrac%7B6.106%20%5Ctimes%2010%5E%7B-3%7D%7D%7Bx%5Ctimes%200.1095%5E%7B6%7D%7D%20%3D%202.0%20%5Ctimes%2010%5E%7B8%7D%5C%5C%5C%5C6.106%20%5Ctimes%2010%5E%7B-3%7D%20%3D%202.0%20%5Ctimes%2010%5E%7B8%7D%5Ctimes%200.1095%5E%7B6%7Dx%3D%20345.1x%5C%5Cx%3D%20%5Cdfrac%7B6.106%20%5Ctimes%2010%5E%7B-3%7D%7D%7B345.1%7D%20%3D%201.77%20%5Ctimes%2010%5E%7B-5%7D%5C%5C%5C%5C%5Ctext%7BThe%20concentration%20of%20Ni%24%5E%7B2%2B%7D%24%20at%20equilibrium%20is%20%24%5Clarge%20%5Cboxed%7B%5Cmathbf%7B1.77%20%5Ctimes%2010%5E%7B-5%7D%7D%5Ctextbf%7B%20mol%2FL%7D%7D%24%7D)
Answer:
(D) The particles of matter are arranged in different ways for the different states.
Explanation:
The particles of matter arrange differently based on the different states
They don't stay the same for each state. They have to change depending on certain things.
25 g of NH₃ will produce 47.8 g of (NH₄)₂S
<u>Explanation:</u>
2 NH₃ + H₂S ----> (NH₄)₂S
Molecular weight of NH₃ = 17 g/mol
Molecular weight of (NH₄)₂S = 68 g/mol
According to the balanced reaction:
2 X 17 g of NH₃ produces 68 g of (NH₄)₂S
1 g of NH₃ will produce 
g of (NH₄)₂S
25g of NH₃ will produce 
of (NH₄)₂S
= 47.8 g of (NH₄)₂S
Therefore, 25 g of NH₃ will produce 47.8 g of (NH₄)₂S
Answer:
Since there are 3 Hydrogen atoms present, the formula mass of H is 1.0 × 3 = 3.0 g/mol. Therefore, by adding them up, the formula mass of ammonia is: [14.0 g/mol + 3.0 g/mol] = 17.0 g/mol.
Answer:
1. A. True
2. A. True
3. B. False
4. A. True
5. B. False
Explanation:
1. The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas. A. True. The pressure of an ideal gas is higher than the one that would exert a real gas.
2. The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other. A. True. The intermolecular forces are negligible.
3. The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be about 1 mL. B. False. The volume of the gas particles is negligible.
4. The molecules in a real gas have finite volumes and do exert forces on each other, thus real gases do not conform to some of the assumptions of an ideal gas as stated by the kinetic molecular theory. A. True. We cannot apply ideal gas laws to real gases.
5. The average kinetic energy of a collection of gas particles is assumed to be inversely proportional to the Kelvin temperature of the gas. B. False. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.
