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3 years ago

What do I write? Please hurry

Chemistry

1 answer:

scoundrel [369]3 years ago

5 0

Answer:

Plants wilt when the turgor turns to zero. From diminished water in cells. The rate of water being lost is greater then the water being absorbed.

Something like this. NOT EXACTLY THIS this is just an example.

I didn't know anything about this topic but I looked it up. For the other words I would look up the other words and see what they have to do with plants withering.

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What do these substances have in common?

Akimi4 [234]

They are compounds Good Luck!

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3 years ago

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The Dew Point... a. is the same as temperature when the relative humidity is 100%. b. can only be given in Kelvin degrees. c. is

telo118 [61]

Answer:

Option (A)

Explanation:

The dew point refers to the temperature at which the amount of water vapor present in the air is so high that the relative humidity becomes 100%, and with the increasing rate of cooling, the condensation process takes place and dew is formed.

So for dew point to occur, the air temperature must reach a condition where the air is fully saturated or the relative humidity is 100%.

Thus, the correct answer is option (A).

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3 years ago

What happens to the number of valence electrons as you move from left to right in the periodic table?

fomenos

Valence electrons increases

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3 years ago

Please help meee! Chemistry!

Leya [2.2K]

P=18000000/6 zeros. not sure how to do rest

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3 years ago

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A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. the total heat capacity of the calorimeter plus water w

Sladkaya [172]

Answer: Th enthalpy of combustion for the given reaction is 594.244 kJ/mol

Explanation: Enthalpy of combustion is defined as the decomposition of a substance in the presence of oxygen gas.

W are given a chemical reaction:

$Mg(s)+\frac{1}{2}O_2(g)\rightarrow MgO(s)$

$c=5760J/^oC$

$\Delta T=0.570^oC$

To calculate the enthalpy change, we use the formula:

$\Delta H=c\Delta T\\\\\Delta H=5760J/^oC\times 0.570^oC=3283.2J$

This is the amount of energy released when 0.1326 grams of sample was burned.

So, energy released when 1 gram of sample was burned is = $\frac{3283.2J}{0.1326g}=24760.181J/g$

Energy 1 mole of magnesium is being combusted, so to calculate the energy released when 1 mole of magnesium ( that is 24 g/mol of magnesium) is being combusted will be:

$\Delta H=24760.181J/g\times 24g/mol\\\\\Delta H=594244.3J/mol\\\\\Delta H=594.244kJ/mol$

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3 years ago