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Artist 52 [7]
3 years ago
10

How can the rate of this reaction be increased

Chemistry
1 answer:
SOVA2 [1]3 years ago
7 0

Answer:

If you increase the concentration of a reactant, there will be more of the chemical present. More reactant particles moving together allow more collisions to happen and so the reaction rate is increased. The higher the concentration of reactants, the faster the rate of a reaction will be.

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Differentiate between the following terms.
Lorico [155]

Answer:

a.reducing agent reduces other elements and make itself oxidized

b.Oxidizing agent reduces itself and make other element oxidized

c.Oxidation state is apparent charge on an atom

Explanation:

7 0
3 years ago
Why does surface area of a reactant influence the rate of the reaction?
telo118 [61]

because it can influence how frequently and sufficiently the particles collide depending on the space it has to do so, for example a large surface area would be have a slower rate of reaction and a lower temperature. (the rate of reaction in terms of concentration, it is diffused from high to low) 
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3 years ago
What volume of H2O is formed at stp when 6.0g of Al is treated with excess NaOH? NaOH + Al + H2O —-> NaAl(OH)4 + H2 (g)
ioda

this is the formula and answer of this question

8 0
3 years ago
Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas
Sergio039 [100]

Answer:

It's nitrogen

Explanation:

cuz it has valence 3 and  a diatomic gas at room temperature

5 0
3 years ago
If the observed value for a density is 0.80 g/mL and the accepted value is 0.70 g/mL what is the percent error?
kvv77 [185]

Answer:

<h2>The answer is 14.29 %</h2>

Explanation:

The percentage error of a certain measurement can be found by using the formula

P(\%) =  \frac{error}{actual \:  \: number}  \times 100\% \\

From the question

actual density = 0.70 g/mL

error = 0.8 - 0.7 = 0.1

So we have

P(\%) =  \frac{0.1}{0.7}  \times 100 \\  = 14.285714...

We have the final answer as

<h3>14.29 %</h3>

Hope this helps you

4 0
3 years ago
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