Answer:
- <u><em>Option D. qsys = - qsurr</em></u>
Explanation:
The symbol q is used to denote heat energy.
Considering positive the heat absorbed and negative the heat released:
- <em>qsys</em> is the heat absorbed by the systme
- <em>qsurr</em> is the heat absorbed by the surroundings
When the system does not do work on or receive work from the surroundings, the first law of thermodynamics states that:
- <em>qsys </em>+ <em>qsurr</em> = 0
From which:
- <em>qsys = - qsurr ← </em>answer
That is the option D.
That means that, the heat abosorbed by the system (if <em>qsys</em> is positive) equals the heat released by the surroundings, or the heat released by the system (if <em>qsys</em> is negative) equals the heat absorbed by the surroundings.
Answer is: the enthalpy is -4383.2 kJ.
Reaction 1: 2M(s) + 6HCl(aq) → 2MCl₃(aq) + 3H₂(g); ΔrH₁ = -725.0 kJ.
Reaction 2: HCl(g) → HCl(aq); ΔrH₂ = -74.8 kJ.
Reaction 3: H₂(g) + Cl₂(g) → 2HCl(g); ∆rH₃ = -1845.0 kJ.
Reaction 4: MCl₃(s) → MCl₃(aq); ΔrH₄ = -476.0 kJ.
Reaction 5: 2M(s) + 3Cl₂(g) → 2MCl₃(s); ΔrH₅ = ?
Using Hess's law (substances that appear in the left and right side of the first, second, third and fourth reaction must cancel out to get fifth reaction):
ΔrH₅ = ΔrH₁ - 6 · ΔrH₂ + 3 · ΔrH₃ - 3 · ΔrH₄.
ΔrH₅ = -725 kJ - 6 · (-74.8 kJ) + 3 · (-1845 kJ) - 3 · (-476 kJ).
ΔrH₅ = -4383.2 kJ.
The number of mole will be 65.81 mole.
An ideal gas would be one for which both the overall volume of the molecules and even the forces that exist between them are so negligible as to have no influence on the behavior of something like the gas.
Number of ideal gas can be calculated by using the formula:
PV = nRT
where, p is pressure, n is number of mole, R is gas constant and T is temperature.
Given data:
V= 1750 = 1750 L
P = 125,000 p = 1.2 atm
R = 0.082 L /mole kelvin
T = 273+127 = 400 K
Now, put the value of given data in above equation.
1.23atm x 1750L = n x 0.0820atm x Liter/ mole x kelvin x 400K
n = 65.81 mole.
Therefore, the number of mole will be 65.81 mole
To know more about mole
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Answer:
K = 8.1 x 10⁻³
Explanation:
We are told here that these gas phase reactions are both elementary processes, thus the reactions forward and reverse are both first order:
A→B Rate(forward) = k(forward) x [A]
and for
B→A Rate(reverse) = k(reverse) x [B]
At equilibrium we know the rates of the forward and reverse reaction are equal, so
k(forward) x [A] = k(reverse) x [B] for A(g)⇌B(g)
⇒ k(forward) / k(reverse) = [B] / [A] = K
4.7 x 10⁻³ s⁻1 / 5.8 x 10⁻¹ s⁻¹ = 8.1 x 10⁻³ = K
Notice how this answer is logical : the rate of the reverse reaction is greater than the forward reaction ( a factor of approximately 120 times) , and will be expecting a number for the equilibrium constant, K, smaller than one where the reactant concentration, [A], will prevail.
It is worth to mention that this is only valid for reactions which are single, elementary processes and not true for other equilibria.
Sulfuric acid or H2SO4 is a strong acid and when in aqueous solution it dissociates completely into hydronium ions or H+ and to HSO4- ions. The sulfuric acid can donate H+ decreasing the pH of a solution. Hope this answers the question.