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3 years ago

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What two forces act in the nucleus to create a 'nuclear tug-of-war'?

1 answer:

Alex787 [66]3 years ago

5 0

Answer:

Electrostatic repulsion, strong nuclear force

Explanation:

The nucleus consists of protons and neutrons. protons are positively charged while neutrons possess no charge.

Since protons are positively charged, they repel each other strongly (like charges repel). This strong repulsion of like charges makes the nucleus somewhat unstable leading to spontaneous fission of heavy nuclei.

However, an opposing force called nuclear attractive force tends to hold the nucleons together. This attraction occurs when two nucleons are bonded by a particle called a π meson.

Hence, the two forces that act in the nucleus to create a 'nuclear tug-of-war' are electrostatic repulsion and a strong nuclear force.

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If 36.2g of Acetic Acid (HC2H302) was dissolved in 300. mL of water, what is the

uysha [10]

Answer:

2.01 M

Explanation:

Step 1: Calculate the moles of acetic acid (HC₂H₃O₂)

The molar mass of acetic acid is 60.05 g/mol. We will use this data to calculate the moles corresponding to 36.2 g of acetic acid.

$36.2g \times \frac{1mol}{60.05g} = 0.603mol$

Step 2: Convert the volume of solution to liters

We will use the relation 1000 mL = 1 L. We assume that the volume of solution is that of water (300 mL)

$300mL \times \frac{1L}{1000mL} = 0.300L$

Step 3: Calculate the molarity of the solution

The molarity is equal to the moles of solute (acetic acid) divided by the liters of solution

$M = \frac{0.603mol}{0.300L} = 2.01 M$

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Arisa [49]

The answer is false .

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The half life of radon-222 is 3.8 days. How Much of a 100g sample is left after 15.2 days

professor190 [17]

Answer:

6.2 g

Explanation:

In a first-order decay, the formula for the amount remaining after <em>n</em> half-lives is

$N = \frac{N_{0}}{2^{n}}$

where

<em>N</em>₀ and <em>N</em> are the initial and final amounts of the substance

1. Calculate the <em>number of half-lives</em>.

If $t_{\frac{1}{2}} = \text{3.8 da}$

$n = \frac{t}{t_{\frac{1}{2}}} = \frac{\text{15.2 da}}{\text{3.8 da}}= \text{4.0}$

2. Calculate the <em>final mass</em> of the substance.

$\text{N} = \frac{\text{100 g}}{2^{4.0}} = \frac{\text{100 g}}{16} = \text{6.2 g}$

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3 years ago

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joja [24]

Answer:

18.9 moles

Explanation:

We have the following data:

V = 50 L

P = 12.4 atm

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R = 0.082 L.atm/K.mol (it is the gas constant)

We use the ideal gas equation to calculate the number of moles n of the gas:

PV = nRT

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Answer:

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Explanation:

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