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makvit [3.9K]
3 years ago
8

Which of the following is not a step in balancing redox reactions in acidic solution, using the half-reaction method?

Chemistry
2 answers:
schepotkina [342]3 years ago
7 0
B <span>Divide the chemical equation into two half-reaction equations, identifying which half-reaction is oxidation and which is reduction 
</span>
marishachu [46]3 years ago
3 0

Answer:

The answer would be A). H2O and OH- are added as needed to the half-reaction equations to make the number of oxygen and hydrogen atoms balance.

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Explanation:

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What best explains why sodium is more likely to react with another element than an element such as neon
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Neon is a noble gas and has a stable structure (8 valence electrons) -therefore, is not very reactive.

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Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reac
frez [133]

Given :

Compound A reacts with Compound B to form only one product, Compound C.

The usual percent yield of C in this reaction is 40%.

10.0 g of A are reacted with excess Compound B, and 6.4 g of Compound C

To Find :

The theoretical yield of C.

Solution :

We know, % yield is given by :

\%\ yield = \dfrac{actual\ yield}{theoretical\ yield }\times 100

Putting given values , we get :

40 = \dfrac{6.4}{theoretical\ yield }\times 100\\\\theoretical\ yield=\dfrac{6.4\times 100}{40}\\\\theoretical\ yield=16\ g

Therefore, theoretical yield of C is 16 g.

Hence, this is the required solution.

7 0
3 years ago
) Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2is 7
Travka [436]

Answer:

Rate of the reaction is 0.2593 M/s

-0.5186 M/s is the rate of the loss of ozone.

Explanation:

The rate of the reaction is defined as change in any one of the concentration of reactant or product per unit time.

2O_3\rightleftharpoons 3O_2

Rate of formation of oxygen : 7.78\times 10^{-1} M/s

Rate of the reaction(R) =\frac{-1}{2}\frac{d[O_3]}{dt}=\frac{1}{3}\frac{d[O_2]}{dt}

R=\frac{1}{3}\frac{d[O_2]}{dt}

Rate of formation of oxygen=3 × (R)

7.78\times 10^{-1} M/s=3\times R

Rate of the reaction(R): 0.2593 M/s

Rate of the reaction is 0.2593 M/s

Rate of disappearance of the ozone:

R=-\frac{1}{2}\frac{d[O_3]}{dt}

\frac{d[O_3]}{dt}=-2\times R=-2\times 0.2593\times M/s=-0.5186M/s

-0.5186 M/s is the rate of the loss of ozone.

6 0
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