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3 years ago

9

Which statement describes the effect of sorting and recombining genes in sexual reproduction?

1 answer:

Setler79 [48]3 years ago

7 0

The fourth option I think

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6.9 moles of oxygen gas in a fixed volume of 1.33 liters. One of the valves opened and there remains only 1.24 moles oxygen gas.

Romashka [77]

Answer:

The new volume of the gas remains the same. That is new volume of gas is 1.33 litres

Explanation:

This is because gases do not have a definite shape. They therefore take the shape of their containing vessels and hence their volumes are determined by the volume of the container.

For the question above even if some of the gas escapes, as long as there is gas present in the container, its volume remains the same, that is occupies the same space in the container

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2 years ago

A particle that has a negative charge Electrons Protons Non-polarMolecule Neutrons

murzikaleks [220]

Electron

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~~have a beautiful day~~
~davatar~

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3 years ago

Which object forms when a supergiant explodes

klasskru [66]

black hole

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3 years ago

Read 2 more answers

Determine the number of ions produced in the dissociation of the compound listed. BaS

11Alexandr11 [23.1K]

BaS → Ba²⁺ + S²⁻
two types of ions

4 0

3 years ago

Read 2 more answers

When 125 grams of FeO react with 25.0 grams of Al, how many grams of Fe can be produced? FeO + Al → Fe + Al2O3 25.9 g Fe 38.7 g

Serga [27]

<u>Answer:</u> The mass of iron produced will be 77.6 grams

<u>Explanation:</u>

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

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

<u>For FeO:</u>

Given mass of FeO = 125 g

Molar mass of FeO = 71.8 g/mol

Putting values in equation 1, we get:

$\text{Moles of FeO}=\frac{125g}{71.8g/mol}=1.74mol$

<u>For aluminium:</u>

Given mass of aluminium = 25.0 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

$\text{Moles of aluminium}=\frac{25.0g}{27g/mol}=0.93mol$

The given chemical reaction follows:

$3FeO+2Al\rightarrow 3Fe+Al_2O_3$

By Stoichiometry of the reaction:

2 moles of aluminium metal reacts with 3 mole of FeO

So, 0.93 moles of aluminium metal will react with = $\frac{3}{2}\times 0.93=1.395mol$ of FeO

As, given amount of FeO is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium metal is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of aluminium metal produces 3 mole of iron metal

So, 0.93 moles of aluminium metal will produce = $\frac{3}{2}\times 0.93=1.395moles$ of iron metal

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

Molar mass of iron = 55.85 g/mol

Moles of iron = 1.395 moles

Putting values in equation 1, we get:

$1.395mol=\frac{\text{Mass of iron}}{55.85g/mol}\\\\\text{Mass of iron}=(1.395mol\times 55.85g/mol)=77.6g$

Hence, the mass of iron produced will be 77.6 grams

4 0

3 years ago