<u>Answer:</u> The volume of hydrogen gas required for the given amount of ethylene gas is 113 L
<u>Explanation:</u>
At STP:
1 mole of a gas occupies 22.4 L of volume
We are given:
Volume of ethylene = 113 L
For the given chemical equation:

By Stoichiometry of the reaction:
of ethylene reacts with
of hydrogen gas
So, 113 L of ethylene gas will react with =
of hydrogen gas
Hence, the volume of hydrogen gas required for the given amount of ethylene gas is 113 L
Answer:
The pressure of the gas at 23 C is 179.92 kPa.
Explanation:
Gay-Lussac's law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of collisions with the walls increases, that is, the pressure increases. That is, the pressure of the gas is directly proportional to its temperature.
In short, when there is a constant volume, as the temperature increases, the pressure of the gas increases. And when the temperature is decreased, the pressure of the gas decreases.
Gay-Lussac's law can be expressed mathematically as follows:

Studying two states, one initial 1 and the other final 2, it is satisfied:

In this case:
- P1= 310 kPa
- T1= 237 C= 510 K (being 0 C= 273 K)
- P2= ?
- T2= 23 C= 296 K
Replacing:

Solving:

P2= 179.92 kPa
<u><em>The pressure of the gas at 23 C is 179.92 kPa.</em></u>
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<span>Answer:
Correct answers are- Electron affinity decreases; Cl has 7 valence electrons but Na has only 1. So Na is going to lose its e, Cl is going to gain an e.</span>