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3 years ago

Based in the rules of John Dalton, what is a possible hypothesis that could be tested in the Atomic Theory lab?

2 answers:

8 0

After many experiments and many different approaches to the question, the scientist may be able to develop a theory. The theory explains why nature behaves in the way described by the natural law. It answers not only the original question, but also any other questions that were raised during the process. The theory also predicts the results of further experiments, which is how it is checked. Theories are not the end of the process.

Schach [20]3 years ago

4 0

Answer:

Dalton's atomic model can be used to explaing the mass concervation withing an chemical reaction.

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The atomic number tells us how many __ or __ an element contains.

CaHeK987 [17]

Answer:-
Electrons or Protons

Explanation:-
Atomic number (Z) is defined as:
>>“The total number of protons in the nucleus of an atom is called atomic number”. All atoms of an element have the same number of protons and electrons.
>>“The total number of protons in the nucleus or electrons revolving around the nucleus of an atom”.
Example:
For instance, Hydrogen has the Atomic number(Z) 1.
Helium has the atomic number 2.
Oxygen has the atomic number 8.
| Note | Atomic number is represented by “Z”. And some ppl don’t consider the 2nd definition it’s upto u to do both or the standard one.

5 0

3 years ago

Henry finds an element that is light blue, breaks easily in his hand, and does not reflect light. How should Henry classify the

pshichka [43]

Answer:

The options are not given, here are the options.

metal

a. Metal

b. a metalloid

c. a non-metal

d. a gas

The correct option is C.

Non metal

Explanation:

Henry should classify it as non metals because non metals are substances or elements that are poor conductors of heat and electricity they break easily I .e meaning they lack the ducibility of metals, meaning they cannot be stretched, they are brittle, they are not shiny and does not reflect light, they have high electronegativities that is they have atoms that can hold electrons to what they have.

4 0

3 years ago

A binary compound created by reaction of bismuth and an unknown element E contains 52.07% Bi and 47.93% E by mass. If the formul

yulyashka [42]

Answer:

Atomic mass of E is 128.24

Explanation:

The percentage composition by mass of an element in a compound is given by dividing the mass of the element by the total mass of the compound and expressing it as a percentage.

In this case; the compound Bi₂E₃

Percentage composition of bismuth = 52.07%

Percentage composition of E = 47.93%

Mass Bismuth in the compound is (2×208.9804) = 417.96 g

Therefore,

To calculate the atomic mass of E

52.07% = 417.96 g

47.93% = ?

= (47.93 × 417.96 ) ÷ 52.07 %

= 384.729

E₃ = 384.729

Therefore; E = 384.729 ÷ 3

= 128.24

The atomic mass of E is 128.24

6 0

3 years ago

How many grams of zinc would be required to produce 9.65g of zinc hydroxide

Effectus [21]

The question is incomplete, here is the complete question:

How many grams of zinc would be required to produce 9.65g of zinc hydroxide

Zn+2MnO₂+H₂O→Zn(OH)₂+Mn₂O₃

Answer: The mass of zinc required is 6.35 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of zinc hydroxide = 9.65 g

Molar mass of zinc hydroxide = 99.4 g/mol

Putting values in equation 1, we get:

$\text{Moles of zinc hydroxide}=\frac{9.65g}{99.4g/mol}=0.0971mol$

The given chemical equation follows:

$Zn+2MnO_2+H_2O\rightarrow Zn(OH)_2+Mn_2O_3$

By Stoichiometry of the reaction:

1 mole of zinc hydroxide is produced from 1 mole of zinc

So, 0.0971 moles of zinc hydroxide will be produced from = $\frac{1}{1}\times 0.0971=0.0971mol$ of zinc

Now, calculating the mass of zinc from equation 1, we get:

Molar mass of zinc = 65.4 g/mol

Moles of zinc = 0.0971 moles

Putting values in equation 1, we get:

$0.0971mol=\frac{\text{Mass of zinc}}{65.4g/mol}\\\\\text{Mass of zinc}=(0.0971mol\times 65.4g/mol)=6.35g$

Hence, the mass of zinc required is 6.35 grams

6 0

3 years ago

Calculate the pressure of 3.2 moles of an ideal gas that occupies a volume of 87 m3 at a temperature of 312 K.

Anestetic [448]

Answer:

P = 0.0009417 atm

Or,

P = 9.417 × 10⁻⁴ atm

Or,

P = 0.0954157 kPa

Or,

P = 0.715677 mmHg (Torr)

Explanation:

Data Given:

Moles = n = 3.2 mol

Temperature = T = 312 K

Pressure = P = ?

Volume = V = 87 m³ = 87000 L

Formula Used:

Let's assume that the gas is acting as an Ideal gas, the according to Ideal Gas Equation,

P V = n R T

where; R = Universal Gas Constant = 0.082057 atm.L.mol⁻¹.K⁻¹

Solving Equation for P,

P = n R T / V

Putting Values,

P = (3.2 mol × 0.082057 atm.L.mol⁻¹.K⁻¹ × 312 K) ÷ 87000 L

P = 0.0009417 atm

Or,

P = 9.417 × 10⁻⁴ atm

Or,

P = 0.0954157 kPa

Or,

P = 0.715677 mmHg (Torr)

4 0

3 years ago

Read 2 more answers