Democritus of Abdera, John Dalton , Niels Bohr, Rutherford

Chemistry

1 answer:

Temka [501]11 months ago

6 0

Niels Bohr and Rutherford model of an atom are best to understand the quantum chemistry.

<h3>What are Niels Bohr and Rutherford model of an atom?</h3>

Niels Bohr explains about the particle behavior of an atom and gives account about the energy level or shells of an atom and hydrogen spectrum too.

Rutherford discovers the nucleus of an atom and identified that the mass of an atom is focused at the center oof an atom and proton is positively charged.

Therefore, Niels Bohr and Rutherford model of an atom are best to understand the quantum chemistry.

Learn more about Niels Bohr and Rutherford model of an atom, here:

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Please help me with my regents practice :((

BlackZzzverrR [31]

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Explanation:

8 0

2 years ago

6. How many moles of water would require 92.048 kJ of heat to raise its temperature from 34.0 °C to 100.0 °C? (3 marks)

scoray [572]

Taking into account the definition of calorimetry, 0.0185 moles of water are required.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

So, the equation that allows to calculate heat exchanges is:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

<h3>Mass of water required</h3>

In this case, you know:

Heat= 92.048 kJ
Mass of water = ?
Initial temperature of water= 34 ºC
Final temperature of water= 100 ºC
Specific heat of water = 4.186 $\frac{J}{gC}$

Replacing in the expression to calculate heat exchanges:

92.048 kJ = 4.186 $\frac{J}{gC}$ × m× (100 °C -34 °C)

92.048 kJ = 4.186 $\frac{J}{gC}$ × m× 66 °C

m= 92.048 kJ ÷ (4.186 $\frac{J}{gC}$ × 66 °C)

<u><em>m= 0.333 grams</em></u>

<h3>Moles of water required</h3>

Being the molar mass of water 18 $\frac{g}{mole}$ , that is, the amount of mass that a substance contains in one mole, the moles of water required can be calculated as: