Answer:
Total pressure at equilibrium is 0.2798atm.
Explanation:
For the reaction:
H₂S(g) ⇄ H₂(g) + S(g)
Kp is defined as:
If initial pressure of H₂S is 0.150 atm, equilibrium pressures are:
H₂S(g): 0.150atm - x
H₂(g): x
S(g): x
Replacing in Kp:
X² = 0.1251 - 0.834X
X² + 0.834X - 0.1251 = 0
Solving for X:
X = -0.964 → False solution: There is no negative pressures
X = 0.1298
Thus, pressures are:
H₂S(g): 0.150atm - 0.1298atm = <em>0.0202atm</em>
H₂(g): <em>0.1298atm</em>
S(g): <em>0.1298atm</em>
Thus, total pressure in the container at equilibrium is:
0.0202atm + 0.1298atm + 0.1298atm = <em>0.2798atm</em>
Answer:
dihydrogen dioxide, hydrogen dioxide, hydrogen oxide, oxydol, peroxide, H 2 O 2.
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Explanation:
Equation of reaction:
CO + 2H₂ ⇒ CH₃OH + energy
a. An increase in pressure:
A change in pressure affects only equilibrium involving a gas or gases. Le Chatelier's principle can be used to predict the direction of displacement.
An increase in pressure on an equilibrium system will shift the position of equilibrium to the side having smaller volume and vice-versa
CO + 2H₂ ⇒ CH₃OH + energy
3 moles 1 moles
An increase in pressure will favor the forward reaction to be favored.
b. Addition of H₂:
An in concentration of a specie favors the direction that uses up that specie and lowers its concentration.
Addition of hydrogen gas increases the concentration of amount of substances reacting.
To annul the effect of the reactant, more the product is given. The equilibrium shifts in the forward direction.
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Answer:
Amount of heat required = 2810.5 J
Explanation:
Given data:
Mass of copper = 29.2 g
Initial temperature = 25°C
Final temperature = 275°C
Amount of heat required = ?
Solution:
Specific heat capacity of copper is 0.385 j/g.°C.
Formula:
Q = m×c×ΔT
ΔT = 275°C - 25°C
ΔT = 250°C
Q = 29.2 g × 0.385 j/g.°C ×250°C
Q = 2810.5 J