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3 years ago

What are atoms made up of

Chemistry

2 answers:

jeka943 years ago

6 0

Protons, neutrons, and elections ( don’t know if it’s multiple choice but hope this helps)

faltersainse [42]3 years ago

3 0

Answer:

They are made up of electrons, neutrons and protons

Explanation:

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a sample of ammonia contains 9g hydrogen and 42g nitrogen. another sample contains 5g hydrogen .calculate the amount of nitrogen

balandron [24]

9 g of hydrogen - 42 g of nitrogen
5 g of hydrogen - x g of nitrogen

$9x=42 \cdot 5 \\
9x=210 \\
x \approx 23.33$

The mass of nitrogen in the second sample is 23.33 g.

4 0

4 years ago

Atom with three full orbits What is it

nekit [7.7K]

Answer:

Boron. The answer is boron.

3 0

3 years ago

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If you made a three-dimensional model of an atom and its nucleus, how would you represent the atom? 7th grade

Gemiola [76]

Answer:

it shows the breakdown of the atom

Explanation:

it will show it molecularly

7 0

3 years ago

The Lewis dot model of a molecule is shown. A visual diagram of a PCl3 molecule is shown. Phosphorous is the central atom with a

Nostrana [21]

The answer is B. Each chlorine has three non-bonded pairs and one bonded pair of electrons.

I just took the test and it was correct! 5/5 :)

8 0

4 years ago

Read 2 more answers

Consider the reaction. 2 HBr(g) ¡ H2(g) + Br2(g) a. Express the rate of the reaction in terms of the change in concentration of

Studentka2010 [4]

Answer :

(A) The rate expression will be:

$Rate=-\frac{1}{2}\frac{d[HBr]}{dt}=+\frac{d[H_2]}{dt}=+\frac{d[Br_2]}{dt}$

(B) The average rate of the reaction during this time interval is, 0.00176 M/s

(C) The amount of Br₂ (in moles) formed is, 0.0396 mol

Explanation :

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The given rate of reaction is,

$2HBr(g)\rightarrow H_2(g)+Br_2(g)$

The expression for rate of reaction :

$\text{Rate of disappearance of }HBr=-\frac{1}{2}\frac{d[HBr]}{dt}$

$\text{Rate of disappearance of }H_2=+\frac{d[H_2]}{dt}$

$\text{Rate of formation of }Br_2=+\frac{d[Br_2]}{dt}$

Part A:

The rate expression will be:

$Rate=-\frac{1}{2}\frac{d[HBr]}{dt}=+\frac{d[H_2]}{dt}=+\frac{d[Br_2]}{dt}$

Part B:

$\text{Average rate}=-\frac{1}{2}\frac{d[HBr]}{dt}$

$\text{Average rate}=-\frac{1}{2}\frac{(0.512-0.600)M}{(25.0-0.0)s}$

$\text{Average rate}=0.00176M/s$

The average rate of the reaction during this time interval is, 0.00176 M/s

Part C:

As we are given that the volume of the reaction vessel is 1.50 L.

$\frac{d[Br_2]}{dt}=0.00176M/s$

$\frac{d[Br_2]}{15.0s}=0.00176M/s$

$[Br_2]=0.00176M/s\times 15.0s$

$[Br_2]=0.0264M$

Now we have to determine the amount of Br₂ (in moles).

$\text{Moles of }Br_2=\text{Concentration of }Br_2\times \text{Volume of solution}$

$\text{Moles of }Br_2=0.0264M\times 1.50L$

$\text{Moles of }Br_2=0.0396mol$

The amount of Br₂ (in moles) formed is, 0.0396 mol

8 0

3 years ago