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tatuchka [14]
3 years ago
8

How could natural selection lead to speciation?

Chemistry
1 answer:
Harlamova29_29 [7]3 years ago
6 0

Answer:

Speciation can be driven by evolution, which is a process that results in the accumulation of many small genetic changes called mutations in a population over a long period of time. ... Natural selection can result in organisms that are more likely to survive and reproduce and may eventually lead to speciation.

I hope it's helpful!

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When many atoms are split in a chain reaction, a large explosion occurs. This is an example of what type of energy conversion? (
lara31 [8.8K]

Answer:

I think is chemical and nuclear

8 0
3 years ago
Read 2 more answers
H2 is an example of? A. a molecule B. an element or C. both a molecule and an element.
lesya [120]

Answer:

The answer is both molecule and an element

Hydrogen is the chemical element with the symbol H and atomic number 1. ... At standard conditions hydrogen is a gas of diatomic molecules having the formula H2. It is colorless, odorless, non-toxic, and highly combustible.

Explanation:

7 0
2 years ago
What has a higher lattice energy? MgS or BaF2
irinina [24]

Answer:

The lattice energy of MgS is 4 times larger than that of NaCl

Explanation:

because, MgS has a higher charge that is Mg2+,S2− M g 2 + , S 2 − than NaCl (Na+,Cl−) ( N a + , C l − ) .

3 0
2 years ago
What is the quantity of heat (in kJ) associated with cooling 185.5 g of water from 25.60°C to ice at -10.70°C?Heat Capacity of S
Cerrena [4.2K]

Taking into account the definition of calorimetry, sensible heat and latent heat,  the amount of heat required is 37.88 kJ.

<h3>Calorimetry</h3>

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

<h3>Sensible heat</h3>

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

<h3>Latent heat</h3>

Latent heat is defined as the energy required by a quantity of substance to change state.

When this change consists of changing from a solid to a liquid phase, it is called heat of fusion and when the change occurs from a liquid to a gaseous state, it is called heat of vaporization.

  • <u><em>25.60 °C to 0 °C</em></u>

First of all, you should know that the freezing point of water is 0°C. That is, at 0°C, water freezes and turns into ice.

So, you must lower the temperature from 25.60°C (in liquid state) to 0°C, in order to supply heat without changing state (sensible heat).

The amount of heat a body receives or transmits is determined by:

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.

In this case, you know:

  • c= Heat Capacity of Liquid= 4.184 \frac{J}{gC}
  • m= 185.5 g
  • ΔT= Tfinal - Tinitial= 0 °C - 25.60 °C= - 25.6 °C

Replacing:

Q1= 4.184 \frac{J}{gC}× 185.5 g× (- 25.6 °C)

Solving:

<u><em>Q1= -19,868.98 J</em></u>

  • <u><em>Change of state</em></u>

The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to

Q = m×L

where L is called the latent heat of the substance and depends on the type of phase change.

In this case, you know:

n= 185.5 grams× \frac{1mol}{18 grams}= 10.30 moles, where 18 \frac{g}{mol} is the molar mass of water, that is, the amount of mass that a substance contains in one mole.

ΔHfus= 6.01 \frac{kJ}{mol}

Replacing:

Q2= 10.30 moles×6.01 \frac{kJ}{mol}

Solving:

<u><em>Q2=61.903 kJ= 61,903 J</em></u>

  • <u><em>0 °C to -10.70 °C</em></u>

Similar to sensible heat previously calculated, you know:

  • c = Heat Capacity of Solid = 2.092 \frac{J}{gC}
  • m= 185.5 g
  • ΔT= Tfinal - Tinitial= -10.70 °C - 0 °C= -10.70 °C

Replacing:

Q3= 2.092 \frac{J}{gC} × 185.5 g× (-10.70) °C

Solving:

<u><em>Q3= -4,152.3062 J</em></u>

<h3>Total heat required</h3>

The total heat required is calculated as:  

Total heat required= Q1 + Q2 +Q3

Total heat required=-19,868.98 J + 61,903 J -4,152.3062 J

<u><em>Total heat required= 37,881.7138 J= 37.8817138 kJ= 37.88 kJ</em></u>

In summary, the amount of heat required is 37.88 kJ.

Learn more about calorimetry:

brainly.com/question/14057615?referrer=searchResults

brainly.com/question/24988785?referrer=searchResults

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brainly.com/question/13959344?referrer=searchResults

brainly.com/question/14309811?referrer=searchResults

brainly.com/question/23578297?referrer=searchResults

7 0
2 years ago
How many formula units of sodium chloride (NaCl) may theoretically be produced from 13.0 g FeCl3?
algol [13]

Answer:

1.445\times 10^{23} formula units of sodium chloride can be formed from 13.0 gram of ferric chloride.

Explanation:

Mass of ferric chloride = 13.0 g

Moles of ferric chloride = \frac{13.0 g}{162.5 g/mol}=0.08 mol

1 mole of ferric chloride has three moles of chloride ions.Then 0.08 moles of ferric chloride will have :

3\times 0.08 mol=0.24 mol of chloride

Na^++Cl^-\rightarrow NaCl

1 mole of sodium ion reacts with 1 mole of chloride ion to form 1 mole of NaCl. Then 0.24 moles of chloride ion will give:

\frac{1}{1}\times 0.24 mol=0.24 mol of NaCl

1 mole = N_A=6.022\times 10^{23} molecules/ atoms

Number of NaCl molecules in 0.24 moles :

=6.022\times 10^{23}\times 0.24=1.445\times 10^{23} molecules

1.445\times 10^{23} formula units of sodium chloride can be formed from 13.0 gram of ferric chloride.

4 0
3 years ago
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