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3 years ago

Which trait will an organism that receives one dominant gene and one recessive gene most

Chemistry

2 answers:

velikii [3]3 years ago

8 0

Answer:

The dominant gene - such as brown hair or brown hair

Explanation:

Dominant refers to the relationship between two versions of a gene. Individuals receive two versions of each gene, known as alleles, from each parent. If the alleles of a gene are different, one allele will be expressed; it is the dominant gene. The effect of the other allele, called recessive, is masked. A person with two dominant or two recessive alleles for a trait is "homozygous." A person with one dominant and one recessive allele for a trait is "heterozygous." Because a boy inherits only one X-chromosome, if there is a recessive gene on that X-chromosome, the gene is expressed.

serious [3.7K]3 years ago

4 0

Answer: dominant

explanation: The dominant Gene wins because it overpowers the recessive gene.

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Which of the following is true about subatomic particles?

galben [10]

Answer:

Explanation:

neutrons and protons have the mass nearly 1.67*10-24 g

but neutrons have no charge.. protons are positively charged

6 0

2 years ago

Assume you are working for a chemical company and are responsible for growing a yeast culture that produces ethanol. The yeasts

romanna [79]

Answer:

Respiration might occur in the presence and absence of oxygen known as the aerobic respiration and anaerobic respiration. The ATP molecules are produced more in number in aerobic respiration.

The yeast has the ability to undergo the process of anaerobic respiration and its end product are alcohol, carbon dioxide and 2 moles of ATP. The yeast is grown on maltose medium but unable to produce alcohol because of the presence of oxygen in the medium. The oxygen might acts as poison or inhibit the process of anaerobic respiration.

6 0

3 years ago

How many moles of methanol must be added to 4.50 kg of water to lower its freezing point to -11.0 ∘c? for each mole of solute, t

DochEvi [55]

Given:

Mass of solvent water = 4.50 kg

Freezing point of the solution = -11 C

Freezing point depression constant = 1.86 C/m

To determine:

Moles of methanol to be added

Explanation:

The freezing point depression ΔTf is related to the molality m through the constant kf, as follows:

ΔTf = kf*m

where ΔTf = Freezing point of pure solvent (water) - Freezing pt of solution

ΔTf = 0 C - (-11.0 C) = 11.0 C

m = molality = moles of methanol/kg of water = moles of methanol/4.50 kg

11.0 = 1.86 * moles of methanol/4.50

moles of methanol = 26.613 moles

Ans: Thus around 26.6 moles of methanol should be added to 4.50 kg of water.

3 0

3 years ago

Which of the following elements is likely to show additional stability in its electronic configurations because of filled and ha

kodGreya [7K]

Ah is gold and Rh is rhodium and Os is osmium and Ir iridium

3 0

2 years ago

If you have a 1500 g aluminum pot, how much heat energy is needed to raise its temperature by 100°C?

Nataly [62]

The heat energy required to raise the temperature of 1500 g of aluminium pot by 100°C is 135 kJ.

The heat energy required to raise the temperature of 1500 g of copper pot by 100 °C is 57.75 kJ.

Explanation:

The heat energy required to raise the temperature of any body can be obtained from the specific heat formula. As this formula states that the heat energy required to raise the temperature of the body is directly proportional to the product of mass of the body, specific heat capacity of the material and temperature change experienced by the material.

So in this problem, the mass of the aluminium is given as m = 1500 g, the specific heat of the aluminium is 0.900 J/g °C. Then as it is stated that the temperature is raised by 100 °C, so the pots are heat to increase by 100 °C from its initial temperature. This means the difference in temperature will be 100°C (ΔT = 100°C).

Then, the heat energy required to raise the temperature will be

$q = m*c*del T = 1500 * 0.900 * 100 = 135000 = 135 kJ$

Thus, the heat energy required to raise the temperature of 1500 g of aluminium pot by 100 °C is 135 kJ.

Similarly, the mass of copper pot is given as 1500 g, the specific heat capacity of copper is 0.385 and the difference in temperature is 100 °C.

Then, the heat energy required to raise its temperature will be

$q = m*c*del T = 1500 * 0.385 * 100 = 57750 = 57.75 kJ$

And the heat energy required to raise the temperature of 1500 g of copper pot by 100°C is 57.75 kJ.

So, the heat energy required to raise the temperature of 1500 g of aluminium pot by 100°C is 135 kJ. And the heat energy required to raise the temperature of 1500 g of copper pot by 100 °C is 57.75 kJ.

8 0

3 years ago