Need the answer asap giving 30 points.
1 answer:
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Answer:
a
No
b
100 mm Hg
Explanation:
From the question we are told that
The vapor pressure of CHCl3, is
The temperature of CHCl3 is
The volume of the container is
The temperature of the container is
The mass of CHCl3 is m = 0.380 g
Generally the number of moles of CHCl3 present before evaporation started is mathematically represented as
Here M is the molar mass of CHCl3 with the value
=>
=>
Generally the number of moles of CHCl3 gas that evaporated is mathematically represented as
Here R is the gas constant with value
So
Given that the number of moles of CHCl3 evaporated is less than the number of moles of CHCl3 initially present , then it mean s that not all the liquid evaporated
At equilibrium the temperature of CHCl3 will be equal to the pressure of air so the pressure at equilibrium is 100 mmHg
Answer:
a. Δ
b. 320.76° C
Explanation:
a.)
we can solve this type of question (i.e calculate Δ , for the gas-phase reaction ) using the Hess's Law.
Δ =
Given from the question, the table below shows the corresponding Δ for each compound.
Compound
Liquid EO -77.4
-74.9
-110.5
If we incorporate our data into the above previous equation; we have:
Δ = (-110.5 kJ/mol + (-74.9 kJ/mol) ) - (-77.4 kJ/mol)
=
b.)
We are to find the final temperature if the average specific heat capacity of the products is 2.5 J/g°C
Given that:
the specific heat capacity (c) = 2.5 J/g°C
= 93.0°C &
the enthalpy of vaporization (Δ) = 569.4 J/g
If, we recall; we will remember that; Specific Heat Capacity is the amount of heat needed to raise the temperature of one gram of a substance by one kelvin.
∴ the specific heat capacity (c) is given as =
Let's not forget as well, that Δ =
If we substitute Δ for
in the above equation, we have;
specific heat capacity (c) =
Making () the subject of the formula; we have:
=
= 227.76°C +93.0°C
= 320.76°C
∴ we can thereby conclude that the final temperature = 320.76°C