What is the percent by mass of oxygen in carbon dioxide (CO2)?
1 answer:
You might be interested in
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.
Answer: The pH at equivalence point for the given solution is 5.59.
Explanation:
At the equivalence point,
So, first we will calculate the moles of as follows.
= 0.0845 mol
Now, volume of present will be calculated as follows.
Volume =
=
= 0.1891 L
Therefore, the total volume will be the sum of the given volumes as follows.
110 ml + 189.1 ml
= 299.13 ml
or, = 0.2991 L
Now,
= 0.283 M
Chemical equation for this reaction is as follows.
As,
=
=
Now,
=
=
Now, pH will be calculated as follows.
pH =
=
= 5.59
Thus, we can conclude that pH at equivalence point for the given solution is 5.59.