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2 years ago

If an element has a mass number of 52 and an atomic number of 24, how many neutrons does the element have

Chemistry

2 answers:

chubhunter [2.5K]2 years ago

8 0

Answer:

Explanation:

To find the number of neutrons, subtract the number of protons from the mass number. number of neutrons.

Vlada [557]2 years ago

8 0

Answer: 28 neutrons

Explanation:

im just guessing here man

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How many liters is 3.3 moles of a gas?

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Answer:

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Deuterium is an isotope of hydrogen. It has a mass number of two. Which describes a deuterium atom? A. a nucleus of one proton a

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also known as heavy hydrogen) is one of two stable isotopes of hydrogen (the other being protium, or hydrogen-1). The nucleus of deuterium, called a deuteron, contains one proton and one neutron, whereas the far more common protium has no neutron in the nucleus.

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3 years ago

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1. How does the amount of energy in the batteries in a flashlight compare to the total amount of energy given off by the flashli

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1. The total energy in the batteries and the total energy given off by the flashlight through heat and light is equal. This is because of the "Law of the Conservation of Energy." Energy cannot be created or destroyed, only changed in form. This can also be backed with the first law of thermodynamics.

2. A rate of a chemical reaction can be increased by increasing the temperature, or introducing a catalyst.

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3 years ago

A student obtains a 10.0g sample of a white powder labeled as BaCl2. After completely dissolving the powder in 50.0mL of distill

LekaFEV [45]

Answer:

Whether barium chloride solution was pure

Explanation:

We may answer whether barium chloride was pure. The sequence of this experiment might be depicted by the following balanced chemical equations:

$BaCl_2 (aq)\rightarrow Ba^{2+} (aq) + 2 Cl^- (aq)$

$Ba^{2+} (aq) + SO_4^{2-} (aq)\rightarrow BaSO_4 (s)$

Having a total sample of 10.0 grams, we would firstly find the mass percentage of barium in barium chloride:

$\omega_{Ba^{2+}} = \frac{M_{Ba}}{M_{BaCl_2}} = \frac{137.327 g/mol}{208.23 g/mol\cdot 100\% = 65.95 \%$

This means in 10.0 g, we have a total of:

$m_{Ba^{2+}} = 10.0 g\cdot 0.6595 = 6.595 g$ of barium cations.

The precipitate is then formed and we measure its mass. Having its mass determined, we'll firstly find the percentage of barium in barium sulfate using the same approach:

$\omega_{Ba} = \frac{137.327 g/mol}{233.38 g/mol}\cdot 100\% = 58.84 \%$

Multiplying the mass we obtained by the fraction of barium will yield mass of barium in barium sulfate. Then:

if this number is equal to 6.595 g, we have a pure sample of barium chloride;
if this number is lower than 6.595 g, this means we have an impure sample of barium chloride, as we were only able to precipitate a fraction of 6.595 g.

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