1)
Addition polymerization
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Answer: The final temperature of the gas is 7.58 °C.
Explanation: We are given initial and final pressure of the system and we need to find the final temperature of the system.
To calculate it, we use the equation given by Gay-Lussac.
His law states that pressure is directly related to the temperature of the gas.

Or,

where,
= initial pressure = 893 mmHg = 1.175atm (Conversion factor: 1atm = 760mmHg)
= initial temperature = 49.3°C = [49.3 + 273.15]K = 322.45K
= Final pressure = 778mmHg = 1.023atm
= Final temperature = ?°C
Putting values in above equation, we get:

Converting Final temperature from kelvin to degree Celsius.
![T_2=280.73K=[280.73-273.15]^oC=7.58^oC](https://tex.z-dn.net/?f=T_2%3D280.73K%3D%5B280.73-273.15%5D%5EoC%3D7.58%5EoC)
Hence, the final temperature of the gas is 7.58 °C.
Answer:

Explanation:
Whenever a question asks you, "What is the concentration after a given time?" or something like that, you must use the appropriate integrated rate law expression.
The reaction is 2nd order, because the units of k are L·mol⁻¹s⁻¹.
The integrated rate law for a second-order reaction is
![\dfrac{1}{\text{[A]}} =\dfrac{1}{\text{[A]}_{0}}+ kt](https://tex.z-dn.net/?f=%5Cdfrac%7B1%7D%7B%5Ctext%7B%5BA%5D%7D%7D%20%3D%5Cdfrac%7B1%7D%7B%5Ctext%7B%5BA%5D%7D_%7B0%7D%7D%2B%20kt)
Data:
k = 2.4 × 10⁻²¹ L·mol⁻¹s⁻¹
[A]₀ = 0.0100 mol·L⁻¹
[A] = 0.009 00 mol·L⁻¹
Calculation
:
![\begin{array}{rcl}\dfrac{1}{\text{[A]}} & = & \dfrac{1}{\text{[A]}_{0}}+ kt\\\\\dfrac{1}{0.00900 }& = & \dfrac{1}{0.0100} + 2.4 \times 10^{-21} \, t\\\\111.1&=& 100.0 + 2.4 \times 10^{-21} \, t\\\\11.1& = & 2.4 \times 10^{-21} \, t\\t & = & \dfrac{11.1}{ 2.4 \times 10^{-21}}\\\\& = & \mathbf{4.6 \times 10^{21}}\textbf{ s}\\\end{array}\\\text{It will take $\large \boxed{\mathbf{4.6 \times 10^{21}}\textbf{ s}}$ for the HI to decompose}](https://tex.z-dn.net/?f=%5Cbegin%7Barray%7D%7Brcl%7D%5Cdfrac%7B1%7D%7B%5Ctext%7B%5BA%5D%7D%7D%20%26%20%3D%20%26%20%5Cdfrac%7B1%7D%7B%5Ctext%7B%5BA%5D%7D_%7B0%7D%7D%2B%20kt%5C%5C%5C%5C%5Cdfrac%7B1%7D%7B0.00900%20%7D%26%20%3D%20%26%20%5Cdfrac%7B1%7D%7B0.0100%7D%20%2B%202.4%20%5Ctimes%2010%5E%7B-21%7D%20%5C%2C%20t%5C%5C%5C%5C111.1%26%3D%26%20100.0%20%2B%202.4%20%5Ctimes%2010%5E%7B-21%7D%20%5C%2C%20t%5C%5C%5C%5C11.1%26%20%3D%20%26%202.4%20%5Ctimes%2010%5E%7B-21%7D%20%5C%2C%20t%5C%5Ct%20%26%20%3D%20%26%20%5Cdfrac%7B11.1%7D%7B%202.4%20%5Ctimes%2010%5E%7B-21%7D%7D%5C%5C%5C%5C%26%20%3D%20%26%20%5Cmathbf%7B4.6%20%5Ctimes%2010%5E%7B21%7D%7D%5Ctextbf%7B%20s%7D%5C%5C%5Cend%7Barray%7D%5C%5C%5Ctext%7BIt%20will%20take%20%24%5Clarge%20%5Cboxed%7B%5Cmathbf%7B4.6%20%5Ctimes%2010%5E%7B21%7D%7D%5Ctextbf%7B%20s%7D%7D%24%20for%20the%20HI%20to%20decompose%7D)
Answer:
The coefficient in a balanced chemical equation indicates the mole ratio of both reactants and products.
Explanation:
For example lets consider the reation between Hydrogen and Oxygen to form water:
2H2 + O2 ----------------------- 2H2O
In this reaction, the coefficients of the balanced reaction can be transformed to Mole ratio according to Avogadro's Law which states that at standard temperature and pressure, equal volume of gases contain the same number of moles.
So the mole ratio for the above equation is the ratio of the coefficient:
2moles : 1 mole : 2 moles
Answer:
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