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3 years ago

Please help with 2,3,4 will give brainlist asap

Chemistry

1 answer:

MrRa [10]3 years ago

6 0

Answer:

C2H4 + 3O2 ----> 2CO2 + 2H2O

2FeBr3 + 3H2SO4 ----> Fe2(SO4)3 + 6HBr

2Al + 3F2 -----> 2AlF3

Explanation:

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A variation of the acetamidomalonate synthesis can be used to synthesize serine. The process involves the following steps: Ethox

Alex73 [517]

Answer:

See detailed mechanism in the image attached

Explanation:

The mechanism shown in detail below is the synthesis of serine in steps.

The first step is the attack of the ethoxide ion base on the diethyl acetamidomalonate substrate giving the enolate and formaldehyde.

The second step is the protonation of the oxyanion from (1) above to form an alcohol as shown.

Acid hydrolysis of the alcohol formed in (3) above yields a tetrahedral intermediate, a dicarboxyamino alcohol.

Decarboxylation of this dicarboxyamino alcohol yields serine, the final product as shown in the image attached.

5 0

3 years ago

Zinc metal and aqueous silver nitrate react to give Zn(NO3)2(aq) plus silver metal. When 5.00 g of Zn(s) and solution containing

Fittoniya [83]

Answer : The percent yield is, 83.51 %

Solution : Given,

Mass of Zn = 5.00 g

Mass of $AgNO_3$ = 25.00 g

Molar mass of Zn = 65.38 g/mole

Molar mass of $AgNO_3$ = 168.97 g/mole

Molar mass of Ag = 107.87 g/mole

First we have to calculate the moles of Zn and $AgNO_3$ .

$\text{ Moles of }Zn=\frac{\text{ Mass of }Zn}{\text{ Molar mass of }Zn}=\frac{5.00g}{65.38g/mole}=0.0765moles$

$\text{ Moles of }AgNO_3=\frac{\text{ Mass of }AgNO_3}{\text{ Molar mass of }AgNO_3}=\frac{25.00g}{168.97g/mole}=0.1479moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$Zn+2AgNO_3\rightarrow Zn(NO_3)_2+2Ag$

From the balanced reaction we conclude that

As, 2 mole of $AgNO_3$ react with 1 mole of $Zn$

So, 0.1479 moles of $AgNO_3$ react with $\frac{0.1479}{2}=0.07395$ moles of $Zn$

From this we conclude that, $Zn$ is an excess reagent because the given moles are greater than the required moles and $AgNO_3$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $Ag$

From the reaction, we conclude that

As, 2 mole of $AgNO_3$ react to give 2 mole of $Ag$

So, 0.1479 moles of $AgNO_3$ react to give 0.1479 moles of $Ag$

Now we have to calculate the mass of $Ag$

$\text{ Mass of }Ag=\text{ Moles of }Ag\times \text{ Molar mass of }Ag$

$\text{ Mass of }Ag=(0.1479moles)\times (107.87g/mole)=15.95g$

Theoretical yield of $Ag$ = 15.95 g

Experimental yield of $Ag$ = 13.32 g

Now we have to calculate the percent yield.

$\% \text{ yield}=\frac{\text{ Experimental yield of }Ag}{\text{ Theretical yield of }Ag}\times 100$

$\% \text{ yield}=\frac{13.32g}{15.95g}\times 100=83.51\%$

Therefore, the percent yield is, 83.51 %

7 0

3 years ago

Imagine a balloon is made from a membrane that's permeable to water but not sucrose molecules. How would the concentration of su

Blababa [14]

Answer:

The concentration of sucrose will decrease.

Explanation:

The balloon contains 50% sucrose solution.

Diffusion is the net movement of the substance from the region of the higher concentration to the region of the lower concentration.

Given that the membrane is only permeable to water not sucrose. So, movement of sucrose will not take place. <u>When the balloon is placed in a beaker of water, by the process of diffusion, the water moves from beaker to balloon and thus, the balloon will expand and the concentration of sucrose solution will decrease.</u>

4 0

3 years ago

The temperature of a gas rose from 250K to 350K. At 350K, the volume of the gas was 3.0L. If the pressure did not change, what w

kompoz [17]

That would be (250/350 )* 3 = 2.143 liters to nearest thousandth

6 0

3 years ago

Which of the statements below best describes a metallic bond?

zhenek [66]

I believe a. is the answer.

5 0

3 years ago