Answer:
Technical program - cosmetologist
Answer: the reaction rate of the forward reaction increases (although it is not among the options shown).
Explanation:
1) The equation given is:
CO (g) + Cl₂ (g) ⇄ COCl₂ (g)
2) The forward reaction is:
CO (g) + Cl₂ (g) → COCl₂ (g)
3) The stoichiometry is 1 mole + 1 mole → 1 mole
4) Analysis and conclusion:
The effect of change in the conditions of an equilibrium is foreseen using Le Chatelier's principle.
Le Chatelier's principle states that a system in equilibrium will act trying to compensate the distress applied to the system.
In this case, the distress is increase in pressure.
To compensate the increase in pressure the system must act by reducing the number of moles in the system. Since the forward reaction implies the conversion of two moles of reagents into one mole of product, the more the forward reaction progress the less the number of moles will be present in the system and so the more the compensation of the increase in pressure. So the forward raction is favored by the increase in pressure.
Favoring the forwar reaction means that its rate will incrase,
Answer:
I don't understand any thing
Explanation:
u help me
Here, Molar mass of N2O4 = 92.02 g/mol
So, Number of molecules in 1 mole (92.02 g) = 6.023 * 10²³
Number of molecules in 76.3 g = 6.023 * 10²³ / 92.02 * 76.3
= 6.023 * 10²³ / 1.20
= 5 * 10²³
In short, Your Answer would be approx. 5 * 10²³ molecules
Hope this helps!
Answer:
[H₂] = 1.61x10⁻³ M
Explanation:
2H₂S(g) ⇋ 2H₂(g) + S₂(g)
Kc = 9.30x10⁻⁸ = ![\frac{[H_{2}]^2[S_{2}]}{[H_{2}S]^2}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BH_%7B2%7D%5D%5E2%5BS_%7B2%7D%5D%7D%7B%5BH_%7B2%7DS%5D%5E2%7D)
First we <u>calculate the initial concentration</u>:
0.45 molH₂S / 3.0L = 0.15 M
The concentrations at equilibrium would be:
[H₂S] = 0.15 - 2x
[H₂] = 2x
[S₂] = x
We <u>put the data in the Kc expression and solve for x</u>:
We make a simplification because x<<< 0.0225:
x = 8.058x10⁻⁴
[H₂] = 2*x = 1.61x10⁻³ M
