So just balance the eqn and take the numbers infront of it
take the unknown (the one that the qn is asking for) and ratio it with the known variable
and then put in the mol that you know for the known variable and just do math to get the answer for the unknown
This is an example of a solution. You make a solution by using water as a solvent in which ammonia dissolves.
Answer: Option (a) is the correct answer.
Explanation:
The given data is as follows.
= 4.19 ![kJ/kg ^{o}C](https://tex.z-dn.net/?f=kJ%2Fkg%20%5E%7Bo%7DC)
= 1.9 ![kJ/kg ^{o}C](https://tex.z-dn.net/?f=kJ%2Fkg%20%5E%7Bo%7DC)
Heat of vaporization (
) at 1 atm and
is 2259 kJ/kg
= 0
Therefore, calculate the enthalpy of water vapor at 1 atm and
as follows.
=
+
= 0 + 2259 kJ/kg
= 2259 kJ/kg
As the desired temperature is given
and effect of pressure is not considered. Hence, enthalpy of liquid water at 10 bar and
is calculated as follows.
= ![0 + 4.19 kJ/kg ^{o}C \times (179.9^{o}C - 100^{o}C)](https://tex.z-dn.net/?f=0%20%2B%204.19%20kJ%2Fkg%20%5E%7Bo%7DC%20%5Ctimes%20%28179.9%5E%7Bo%7DC%20-%20100%5E%7Bo%7DC%29)
= 334.781 kJ/kg
Hence, enthalpy of water vapor at 10 bar and
is calculated as follows.
![H^{D}_{vap} = H^{o}_{vap} + C_{p}_{vap} \times (T_{D} - T_{o})](https://tex.z-dn.net/?f=H%5E%7BD%7D_%7Bvap%7D%20%3D%20H%5E%7Bo%7D_%7Bvap%7D%20%2B%20C_%7Bp%7D_%7Bvap%7D%20%5Ctimes%20%28T_%7BD%7D%20-%20T_%7Bo%7D%29)
=
= 2410.81 kJ/kg
Therefore, calculate the latent heat of vaporization at 10 bar and
as follows.
=
= 2410.81 kJ/kg - 334.781 kJ/kg
= 2076.029 kJ/kg
or, = 2076 kJ/kg
Thus, we can conclude that at 10 bar and
latent heat of vaporization is 2076 kJ/kg.
It takes 31 s for 1.27 M H₃PO₄ to decrease its concentration to 7.0% of its initial value following first-order kinetics.
<h3>What is first-order kinetics?</h3>
First-order kinetics occur when a constant proportion of a reactant disappears per unit time.
Let's consider the following first-order kinetics reaction with a rate constant k = 0.086 s⁻¹.
2 H₃PO₄(aq) = P₂O₅(aq) + 3 H₂O(aq)
Given the initial concentation is [H₃PO₄]₀ = 1.27 M, the concentration representing 7.0% of this value is:
[H₃PO₄] = 7.0% × 1.27 M = 0.089 M
We can calculate the time elapsed (t) using the following expression.
ln ([H₃PO₄]/[H₃PO₄]₀) = - k × t
ln (0.089 M/1.27 M) = - 0.086 s⁻¹ × t
t = 31 s
It takes 31 s for 1.27 M H₃PO₄ to decrease its concentration to 7.0% of its initial value following first-order kinetics.
Learn more about first-order kinetics here: brainly.com/question/18916637
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