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3 years ago

16. When a reaction is at equilibrium

Chemistry

1 answer:

Ronch [10]3 years ago

8 0

Answer:

The forward reaction rate is equal to the reverse reaction rate

Explanation:

In many cases, a lot of people might think that equilibrium is a state when a reaction stops. This is not the case, however. Notice that equilibrium reactions are represented by double arrows indicating that two reactions take place simultaneously: both a forward and a reverse reaction.

When equilibrium is reached, the rate of a forward reaction becomes equal to the rate of a reverse reaction. The two reactions don't stop and still take place, just at equal rates. This is the reason why the concentrations of reactants and products are kept constant at equilibrium: the rates of the two reactions are balanced.

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BRAINLIESTTT ASAP!!! PLEASE HELP ME :)<br><br> Describe Chadwick’s work in Chemistry.

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Sir James Chadwick was the scientist who discovered the neutron. The electron and proton had already been found but with the neutron known, we knew everything that made up our universe. He won the 1935 Nobel Peace Prize for his discovery.

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4 years ago

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Method of separate of green solution from leaves and alcohol from warer

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3 years ago

Plastic are made of one type material. why are they not classified as a composite

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3 years ago

Vitamin C has the formula CxHyOz. You burn 0.486 g of the compound in a combustion analysis chamber and isolate 0.728 g of CO2 a

-Dominant- [34]

Answer:

$C_3H_4O_3$

Explanation:

Hello there!

In this case, according to the given information derived from the combustion analysis, it turns out possible for us to realize that all the carbon comes from the CO2 and all the hydrogen from the H2O, it means we can calculate their moles in the vitamin C as shown below:

$n_C=0.728gCO_2*\frac{1molCO_2}{44.01gCO_2}*\frac{1molC}{1molCO_2}=0.0165molC\\\\n_H= 0.198gH_2O*\frac{1molH_2O}{18.02gH_2O}*\frac{2molH}{1molH_2O}=0.0220molH$

Next, we calculate the grams and moles of oxygen from the grams of C and H in the sample:

$m_O=0.486g-0.0165molC*\frac{12.01gC}{1molC} -0.0220molH*\frac{1.01gH}{1molH}\\\\m_O=0.266gO\\\\n_O=0.266gO*\frac{1molO}{16.00gO} =0.0166molO$

Then, we divide the moles of C, H, O by 0.0165 as the fewest moles in order to calculate the correct mole ratios:

$C=\frac{0.0165}{0.0165}= 1\\\\H=\frac{0.0220}{0.0165}= 1.33\\\\O=\frac{0.0166}{0.0165}= 1$

Finally, we turn them into whole number by multiplying by 3 so that the empirical formula is:

$C_3H_4O_3$

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3 years ago

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Part a predict the product and propose a mechanism for the elimination reaction that results when (s)-(1-chloropropyl)benzene is

In-s [12.5K]

Answer:

Propenyl-benzene

Explanation:

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Elimination reaction of solid (1-chloropropyl)-benzene due to the heat in presence of ethanol turns out based on the attached picture in which both the chlorine a the hydrogen in the second carbon go out and subsequently get together to form propenyl-benzene and hydrochloric acid.

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4 years ago