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3 years ago

Answer the following questions ( image) with the given options.

Chemistry

2 answers:

kondor19780726 [428]3 years ago

8 0

Answer:

ans: B) domestic liquid and solid water

wlad13 [49]3 years ago

6 0

Answer:

B. domestic liquid and solid water

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Mention any two factors that determines Cis/Trans Isomerization

kenny6666 [7]

Answer:

1. There most not be rotation within the molecule.

2. Two non identical group must be present in the double bonded carbon atom.

Explanation:

This is because cis/ trans isomerism are that exhibit different structural configurations where the atoms are spartially arranged. They are also refered to as geometric isomers. They cannot be interconverted at room temperature because it requires the bonds to be broken and restructured.

Cis shows that the functional groups on present in the same side which trans isomerism show that the functional groups are on opposite sides.

6 0

3 years ago

How much energy in kilojoules is released when 23.4 g of ethanol vapor at 83.0 ∘C is cooled to -15.0 ∘C ?

slamgirl [31]

Answer : The amount of in kilojoules released is, -5.53 kJ

Explanation :

Formula used :

$q=m\times c\times (T_{final}-T_{initial})$

where,

q = heat released = ?

c = specific heat of ethanol = $2.41J/g^oC$

m = mass of ethanol = 23.4 g

$T_{final}$ = final temperature = $-15.0^oC$

$T_{initial}$ = initial temperature = $83.0^oC$

Now put all the given values in the above formula, we get:

$q=23.4g\times 2.41J/g^oC\times (-15.0-83.0)^oC$

$q=-5526.612J=-5.53\times 10^3J=-5.53kJ$

Therefore, the amount of in kilojoules released is, -5.53 kJ

5 0

4 years ago

if 10.8 moles of hydrogen gas are consumed how many moles of nitrogen gas werw consumed in the reaction

dusya [7]

<em><u>Answer:</u></em>

<h3>look at the balanced chemical equation for this synthesis reaction </h3><h3> S mole ratio between nitrogen gas and hydrogen gas. This means that, regardless of how many moles of nitrogen gas you have, the reaction will always consume twice as many moles of hydrogen gas.</h3><h3 />

8 0

4 years ago

Read 2 more answers

100. mg of an unknown protein are dissolved in enough solvent to make 5.00mL of solution. The osmotic pressure of this solution

PolarNik [594]

<u>Answer:</u> The molar mass of the unknown protein is 6387.9 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

or,

$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 0.0766 atm

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of protein = 100. mg = 0.100 g (Conversion factor: 1 g = 1000 mg)

Molar mass of protein = ?

Volume of solution = 5.00 mL

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[25+273]K=298K$

Putting values in above equation, we get:

$0.0766atm=1\times \frac{0.100\times 1000}{\text{Molar mass of protein}\times 5}\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 298K\\\\\pi=\frac{1\times 0.100\times 1000\times 0.0821\times 298}{0.0766\times 5}=6387.9g/mol$