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3 years ago

7

Describe one conclusion made by Thomson that led to the development of the current atomic theory

1 answer:

lana66690 [7]3 years ago

4 0

He concluded that elecotrons was found in all atoms.:) hope i helped

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Name the following:<br> Simple chemical molecules made of single unit

Stolb23 [73]

Answer:

atom is the answer I think

7 0

3 years ago

Why is it important to collect all data during experiments, rather than make inferences of what will happen?

Paraphin [41]

Answer:

It is important to collect all data first, or else your guesses could purely be the opposite of the right answer. If you make inferences of what might happen, your guesses may be purely fictional, and totally off-topic. During experiments, this step is important.

7 0

3 years ago

What is the percent error when a student measures the volume to be 19.3 liters when

katrin2010 [14]

Answer:

The answer is

<h2>13.84 %</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 volume = 22.4 L

error = 22.4 - 19.3 = 3.1

The percentage error is

$P(\%) = \frac{3.1}{22.4} \times 100 \\ = 13.839285714...$

We have the final answer as

<h3>13.84 %</h3>

Hope this helps you

7 0

3 years ago

I have four neutrons and I'm metallic. Who am<br> I?

Mekhanik [1.2K]

Beryllium has four neutrons

8 0

3 years ago

Read 2 more answers

g The decomposition reaction of A to B is a first-order reaction with a half-life of 2.42×103 seconds: A → 2B If the initial con

Tanzania [10]

Answer:

In 23.49 minutes the concentration of A to be 66.8% of the initial concentration.

Explanation:

The equation used to calculate the constant for first order kinetics:

$t_{1/2}=\frac{0.693}{k}}$ .....(1)

Rate law expression for first order kinetics is given by the equation:

$t=\frac{2.303}{k}\log\frac{[A_o]}{[A]}$ ......(2)

where,

k = rate constant

$t_{1/2}$ =Half life of the reaction = $2.42\times 10^3 s$

t = time taken for decay process = ?

$[A_o]$ = initial amount of the reactant = 0.163 M

[A] = amount left after time t = 66.8% of $[A_o]$

[A]= $\frac{66.8}{100}\times 0.163 M=0.108884 M$

$k=\frac{0.693}{2.42\times 10^3 s}$

$t=\frac{2.303}{\frac{0.693}{2.42\times 10^3 s}}\log\frac{0.163 M}{0.108884 M}$

t = 1,409.19 s

1 minute = 60 sec

$t=\frac{1,409.19 }{60} min=23.49 min$

In 23.49 minutes the concentration of A to be 66.8% of the initial concentration.

6 0

3 years ago