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Len [333]
3 years ago
5

Based on the chemical equation, use the drop down menu to choose the coefficients that will balance the chemical equation:

Chemistry
2 answers:
ivolga24 [154]3 years ago
6 0

Answer: 3O_2(g)\rightarrow 2O_3(g)

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

The balanced chemical equation for the given reaction will be:

3O_2(g)\rightarrow 2O_3(g)

where the (g) stands for the state of reactants and products which is gaseous.

GREYUIT [131]3 years ago
5 0

The answers would be 3 and 2 so the subscripts would both equal 6.

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Some radioactive nuclides have very short half-lives, for example, I-31 has a half-life of approximately 8 days. Pu-234, by comp
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Answer:

Here's what I find.

Explanation:

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About 90 % of the energy is β-radiation and 10 % is γ-radiation. Both forms are highly energetic.

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Plutonium-239

Plutonium-239 is an alpha emitter.

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However, they are extremely dangerous when they are inhaled and get inside cells. They travel first to the blood or lymph system and later to the bone marrow and liver, where they cause up to 1000 times more chromosomal damage than beta or gamma rays.

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3 years ago
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2 years ago
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sleet_krkn [62]

Answer:

Here are a few more examples:

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Explanation:

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Given that the freezing point depression constant for water is 1.86°c kg/mol, calculate the change in freezing point for a 0.907
melamori03 [73]

Answer : The correct answer for change in freezing point = 1.69 ° C

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It is defined as depression in freezing point of solvent when volatile or non volatile solute is added .

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It can be expressed as :

ΔTf = Freezing point of pure solvent - freezing point of solution = i* kf * m

Where : ΔTf = change in freezing point (°C)

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m = molality of solute (m or \frac{mol}{Kg} )

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ΔTf = 1.69 ° C

Hence change in freezing point = 1.69 °C

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3 years ago
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