The ingredients that is important in making plastics is natural gas plant liquids.
Natural gas liquids (NGLs) are components of natural gas which are separated from the gas state in the form of liquids. They many applications including; plastic production, inputs for petrochemical plants, they are also burned for space heat and cooking, and can also be blended into vehicle fuel.
In the manufacturing of plastics, come components of NGLs are used. And for this case, ethane. Ethane is used in the production of ethylene which are passed through pressure and catalyst to be turned to plastics like polythene.
The reason why they are mostly used in the manufacturing plastics than other resources like crude oil is that it is much cleaner.
Learn more about natural gas liquids here:
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Answer:
13mL
Explanation:
Step 1:
The balanced equation for the reaction. This is given below:
HNO3 + KOH —> KNO3 + H2O
From the balanced equation above, we obtained the following data:
Mole ratio of the acid (nA) = 1
Mole ratio of the base (nB) = 1
Step 2:
Data obtained from the question.
This includes the following:
Molarity of the acid (Ma) = 6M
Volume of the acid (Va) =?
Volume of the base (Vb) = 39mL
Molarity of the base (Mb) = 2M
Step 3:
Determination of the volume of the acid.
Using the equation:
MaVa/MbVb = nA/nB, the volume of the acid can be obtained as follow:
MaVa/MbVb = nA/nB
6 x Va / 2 x 39 = 1/1
Cross multiply to express in linear form
6 x Va = 2 x 39
Divide both side by 6
Va = (2 x 39)/6
Va = 13mL
Therefore, the volume of the acid (HNO3) needed for the reaction is 13mL
Answer:
The conversion achieved for the first CSTR impeller is 0.382
Discrepancy = 0.188
Explanation:
The impeller divides the CSTR into 2 equal reactors of volume 500gal
Using V = FaoX/ (-ra)
500gal = Fao×Xa/[(KCao^2( 1 -X1)^2]
500gal = CaoVoX1/ KCao^2(1-X1)
500gal= 500gal × X1'/(1 - X1)^2
(1 -X1)^2 = X1
X1^2 - 3X1 + 1 = 0
X1= 0.382
Conversion achieved in the first CSTR is 0.382
Actual measured CSTR = 57% =57/100=0.57
Discrepancy in the conversions= 0.57 -0.383 =0.188
Answer:
1.94 × 10⁻³
Explanation:
Step 1: Calculate the concentration of H⁺ ions
We will use the definition of pH.
pH = -log [H⁺]
[H⁺] = antilog -pH = antilog -2.32 = 4.79 × 10⁻³ M
Step 2: Calculate the acid dissociation constant (Ka) of the acid
For a monoprotic weak acid, whose concentration (Ca) is 0.0118 M, we can use the following expression.
Ka = [H⁺]²/Ca
Ka = (4.79 × 10⁻³)²/0.0118 = 1.94 × 10⁻³
