This phenomenon is known as the periodic trends in reactivity. It occurs because of the arrangement of electrons in orbitals.
As one moves from left to right across a period, the number of electrons in the outermost shell increases. These outermost electrons are involved in chemical reactions.
Therefore, as the number of outermost electrons increases, the reactivity of the element increases. However, the elements have filled shells, so beyond a certain point, the outermost shell will be full.
The reactivity then decreases as the electrons are no longer available to take part in chemical reactions. Therefore, the reactivity of the elements decreases from left to right in a period and then increases as the outermost shell begins to fill up again.
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This can’t have a answer unless u change them into another number of Delanece
C
The forward and reverse processes would still be ongoing (the system is not still as in the case of static equilibrium), however, the net effect between the two processes is zero. This is what is referred to as dynamic equilibrium.
A closed system, is one that does not exchange matter or energy between it and the environment.
Explanation:
Take an example of a simplest reversible reaction like the following;
A ⇔ B
To get the dynamic equilibrium constant for the reaction we use the following equation;
Keq = [B]eq / [A]eq
Where eq denotes equilibrium.
An example of a reversible reaction where this applies is;
NH₄Cl (s) ⇔ NH₃ (g) + HCl (g)
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Answer: Volume of the gas at STP is 22.53 L.
Explanation:
Given : Volume = 125 mL (as 1 mL = 0.001 L) = 0.125 L
Temperature = ![70^{o}C = (70 + 273) K = 343 K](https://tex.z-dn.net/?f=70%5E%7Bo%7DC%20%3D%20%2870%20%2B%20273%29%20K%20%3D%20343%20K)
Pressure = ![125 kPa = 125 kPa \times \frac{0.01 atm}{1 kPa} = 1.25 atm](https://tex.z-dn.net/?f=125%20kPa%20%3D%20125%20kPa%20%5Ctimes%20%5Cfrac%7B0.01%20atm%7D%7B1%20kPa%7D%20%3D%201.25%20atm)
According to the ideal gas equation, the volume of given nitrogen gas is calculated as follows.
PV = nRT
where,
P = pressure
V = volume
n = number of moles
R = gas constant = 0.0821 L atm/mol K
T = temperature
Substitute the values into above formula as follows.
![1.25 atm \times V = 1 mol \times 0.0821 L atm/mol K \times 343 K\\V = \frac{1 mol \times 0.0821 L atm/mol K \times 343 K}{1.25 atm}\\= \frac{28.1603}{1.25} L\\= 22.53 L](https://tex.z-dn.net/?f=1.25%20atm%20%5Ctimes%20V%20%3D%201%20mol%20%5Ctimes%200.0821%20L%20atm%2Fmol%20K%20%5Ctimes%20343%20K%5C%5CV%20%3D%20%5Cfrac%7B1%20mol%20%5Ctimes%200.0821%20L%20atm%2Fmol%20K%20%5Ctimes%20343%20K%7D%7B1.25%20atm%7D%5C%5C%3D%20%5Cfrac%7B28.1603%7D%7B1.25%7D%20L%5C%5C%3D%2022.53%20L)
Hence, volume of the gas at STP is 22.53 L.
Answer:
2 Atm; 2.016 g
Explanation:
Changing the volume without changing the temperature or mass only changes the pressure. Volume and pressure are inversely proportional so halving the volume will double the pressure.
P = 1 Atm, T = 0 °C are "standard" temperature and pressure (STP). The volume of 1 mole of gas is 22.4 L under these conditions. That means the amount of hydrogen gas in the cylinder is 1 mole, so has a mass of 2.016 g.
After the volume reduction, the pressure is 2 Atm, and the mass remains 2.016 g.