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Airida [17]
3 years ago
10

a chemical company claims that they are able to produce a certain product thermodynamically unfavored process. Explain how this

is possible
Chemistry
1 answer:
KonstantinChe [14]3 years ago
8 0
Thermodynamically favored process are those processes that do not require any assistance from outside the system e.g water boils at 25 degrees. Thermodynamically unfavored processes require assistance from outside to induce the required change for example water doesn't freeze at 15 degrees and therefore for that to happen several factors in the system have to be modified to achieve this. Therefore, there is a possibility of companies to produce product by using thermodynamically unfavored process by inducing changes in the system to achieve desired change or modification.
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Which of these equations is balanced?
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3 years ago
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"A crosslinked copolymer consists of 57 wt% ethylene (C2H4) repeat units and 43 wt% propylene (C3H6) repeat units. Determine the
ch4aika [34]

Explanation:

Percentage ethylene by weight = 57%

Percentage propylene by weight = 43%

Suppose in 100 grams of polymer:

Mass of ethylene = 57 g

Mass of propylene = 43 g

Moles of ethylene = \frac{57 g}{28 g/mol}=2.036 mol

Moles of propylene = \frac{43g}{42g/mol}=1.024 mol

1 mole = N_A =6.022\times 10^{23} molecules/ atoms

Units of ethylene = 2.036 mol\times N_A

Units of propylene = 1.024 mol\times N_A

a) Fraction of ethylene units:

=\frac{2.036 mol\times N_A}{2.306 mol\times N_A+1.024 mol\times N_A}=\frac{509}{765}

b ) Fraction of propylene units:

=\frac{1.024mol\times N_A}{2.306 mol\times N_A+1.024 mol\times N_A}=\frac{256}{765}

3 0
3 years ago
A car accelerates from rest to a speed of 24 m/s in 8 seconds. What is the car's average acceleration
densk [106]

Answer:

3 m/s

Explanation:

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Determine the mass of sodium carbonate required to produce 23.4g of sodium chloride when it reacts with excess hydrochloric acid
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The balanced chemical reaction for the described reaction above is,
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Thus, approximately 21.22 g Na2CO3 is needed for the desired reaction. 
8 0
3 years ago
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