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Gekata [30.6K]
4 years ago
11

To calculate changes in concentration for a system not at equilibrium, the first step is to determine the direction the reaction

will proceed. To do so, we calculate Q and compare it to the equilibrium concentration, K. We can then determine that a reaction will shift to the right if:__________
Chemistry
1 answer:
Viefleur [7K]4 years ago
3 0

Answer:

We can then determine that a reaction will shift to the right if <u><em>Q<K</em></u>

Explanation:

Comparing Q with K allows to find out the status and evolution of the system:

  • If the reaction quotient is equal to the equilibrium constant, Qc = Kc, the system has reached chemical equilibrium.
  • If the reaction quotient is greater than the equilibrium constant, Qc> Kc, the system is not in equilibrium and will evolve spontaneously, decreasing the value of Qc until it equals the equilibrium constant. In this way, the concentrations of the products will decrease and the concentrations of the reagents will increase. In other words, the reverse reaction is favored to achieve equilibrium. Then the system will evolve to the left (ie products will be consumed and more reagents will be formed).
  • If the reaction quotient is less than the equilibrium constant, Qc <Kc, the system is not in equilibrium and will evolve spontaneously increasing the value of Qc until it equals the equilibrium constant. This implies that the concentrations of the products will increase and those of the reagents will decrease. In other words, to achieve balance, direct reaction is favored. Then the reaction will shift to the right, that is, reagents will be consumed and more products will be formed.

In this case, <u><em>we can then determine that a reaction will shift to the right if Q<K</em></u>

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A 15.0 L tank of gas contained at a high pressure of 8.20 • 10^4 torr. The tank is opened and the gas expands into an empty cham
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Answer:

P₂ = 0.205torr

Explanation:

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<em>Where P is pressure and V volume of of 1, initial conditions and 2, final conditions.</em>

P₂ is our incognite

Replacing:

P₁V₁ = P₂V₂

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3 years ago
2.0L of hydrogen gas is mixed with 3.0L of nitrogen gas at STP in a rigid 5.0L vessel. A reaction occurs, producing ammonia gas
IrinaK [193]

Answer:

Moles NH₃: 0.0593

0.104 moles of N₂ remain

Final pressure: 0.163atm

Explanation:

The reaction of nitrogen with hydrogen to produce ammonia is:

N₂ + 3 H₂ → 2 NH₃

Using PV = nRT, moles of N₂ and H₂ are:

N₂: 1atmₓ3.0L / 0.082atmL/molKₓ273K = 0.134 moles of N₂

H₂: 1atmₓ2.0L / 0.082atmL/molKₓ273K = 0.089 moles of H₂

The complete reaction of N₂ requires:

0.134 moles of N₂ × (3 moles H₂ / 1 mole N₂) = <em>0.402 moles H₂</em>

That means limiting reactant is H₂. And moles of NH₃ produced are:

0.089 moles of H₂ × (2 moles NH₃ / 3 mole H₂) = <em>0.0593 moles NH₃</em>

Moles of N₂ remain are:

0.134 moles of N₂ - (0.089 moles of H₂ × (1 moles N₂ / 3 mole H₂)) = <em>0.104 moles of N₂</em>

And final pressure is:

P = nRT / V

P = (0.104mol + 0.0593mol)×0.082atmL/molK×273K / 5.0L

<em>P = 0.163atm</em>

7 0
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What are the standard temperature and pressure conditions enthalpy is usually measured under?
oksian1 [2.3K]

The standard temperature and pressure conditions enthalpy is usually measured under are 1kPa and 273K (option A).

<h3>What is enthalpy?</h3>

Enthalpy in thermodynamics is a measure of the heat content of a chemical or physical system.

Enthalpy is the sum of the internal energy and pressure times volume It can be calculated using the following formula:

H = E + P V

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H = Enthalpy

E = internal energy

P = pressure

V = volume

However, the enthalpy of a substance is usually measured under standard temperature and pressure.

  • The standard temperature is 273 Kelvin or K
  • The standard pressure is 1kPa

Learn more about enthalpy at: brainly.com/question/13996238

#SPJ1

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