Answer:
D. 5.0
Explanation:
Step 1: Write the balanced equation at equilibrium
2 NO₂(g) ⇄ N₂O₄(g)
Step 2: Calculate the concentration equilibrium constant
The concentration equilibrium constant (Kc) is equal to the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.
Kc = [N₂O₄]/[NO₂]² = 0.2 / 0.2² = 5
28.0 x 0.6424 = 18
25.0 x .6424 = 16.1
Mass = 34.1
Answer:
The answer to the question is
The temperature at which the vapor pressure will be 5.00 times higher than it was at 331 K is 353.0797 K.
Explanation:
To solve the question, we make use of the Clausius-Clapeyron equation as follows

Where P₁ = Initial pressure
P₂ = Final pressure
T₁ = Initial temperature = 331 K
T₂ = Final temperature
dvapH = ΔvapH = Heat of vaporization = 70.83 kJ / mol.
R = Universal gas constant = 8.3145. J K⁻¹ mol⁻¹
We are required to find the temperature when P₂ = 5 × P₁
Therefore we have
=
or T₂ =
= 353.0797 K
The vapor pressure be 5.00 times higher than it was at 331 K when the temperature is raised to 353.0797 K.
the answer is c. Gas molecules will never collide with the walls of the container
Answer:
Earth's energy budget describes the balance between the radiant energy that reaches Earth from the sun and the energy that flows from Earth back out to space
Explanation:
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