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Eddi Din [679]
3 years ago
7

Celery stalks immersed in a 0.2 M solution of NaCl for 3 hours become limp and soft. Similar celery stalks immersed in fresh wat

er for 3 hours become stiff and hard. What can be deduced about the celery cells based on this information?
Chemistry
1 answer:
stiv31 [10]3 years ago
5 0

Answer:

The celery cells are hypertonic to freshwater but hypotonic to 0.2M solution of NaCl

Explanation:

<em>A hypertonic solution is one that whose concentration is more than that of the sap of the cell placed in it while a hypotonic solution has lesser concentration compared to the cell sap.</em>

When the surrounding solution of a cell has more concentration than the cell sap, water molecules moves from the cell to the surrounding solution until equal concentration is established between the outer and the inner solution. The cell lose water and become flaccid. Such cell is said to be hypotonic to the surrounding solution.

On the other hand, when the surrounding solution has lower concentration than the cell sap, water moves from the surrounding solution into the cell and as a result, such cell becomes turgid. The cell is said to be hypertonic to the surrounding solution.

Water moves from the cell sap to the surrounding 0.2M NaCl solution, meaning that celery cells are hypotonic to 0.2M NaCl. On the other hand, water moves from surrounding freshwater into the cell, meaning that celery cells are hypertonic to freshwater.

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You observe an exothermic gaseous reaction that is not spontaneous in forward direction at 1 atm and 298K. Which of the followin
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Answer: option (a) is the correct answer

Explanation:

The complete questions says;

You observe an exothermic gaseous reaction that is not spontaneous in forward direction at 1 atm and 298K. Which of the following statements about this reaction is true? a. This reaction will become spontaneous in forward direction at some temperature below 298K. b. This reaction will be spontaneous in forward direction at a higher pressure at 298K. c. This reaction will become spontaneous in forward direction at some temperature above 298K. d. This reaction is never spontaneous. e. The reverse reaction is always spontaneous.

The Answer:

(a). This reaction will become spontaneous in forward direction at some temperature below 298K

Explanation: First of all, we can acknowledge that the reaction seen here is an exothermic one, i.e energy is released in the process outwardly and as a result temperature is reduced during this process of energy loss.

Having understood that scenario, say we reduce it's temperature by ourself than forward reaction favors and after reaching at particular temperature, therefore we can confirm this to be a spontaneous reaction.

Let us use this to confirm what we have been saying.

Given;

ΔG = ΔH - TΔS

here ΔH is negative

it is non spontaneous, which means ΔG is positive so we continuously decraeses it's temperature than at a particular temperature.

The Entropy change becomes positive and reaction becomes spontaneous and ΔG become negative.

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8 0
3 years ago
Using the following reaction (depicted using molecular models), large quantities of ammonia are burned in the presence of a plat
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Answer:

17.65 grams of O2 are needed for a complete reaction.

Explanation:

You know the reaction:

4 NH₃ + 5 O₂ --------> 4 NO + 6 H₂O

First you must know the mass that reacts by stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction). For that you must first know the reacting mass of each compound. You know the values ​​of the atomic mass of each element that form the compounds:

  • N: 14 g/mol
  • H: 1 g/mol
  • O: 16 g/mol

So, the molar mass of the compounds in the reaction is:

  • NH₃: 14 g/mol + 3*1 g/mol= 17 g/mol
  • O₂: 2*16 g/mol= 32 g/mol
  • NO: 14 g/mol + 16 g/mol= 30 g/mol
  • H₂O: 2*1 g/mol + 16 g/mol= 18 g/mol

By stoichiometry, they react and occur in moles:

  • NH₃: 4 moles
  • O₂: 5 moles
  • NO: 4 moles
  • H₂O: 6 moles

Then in mass, by stoichiomatry they react and occur:

  • NH₃: 4 moles*17 g/mol= 68 g
  • O₂: 5 moles*32 g/mol= 160 g
  • NO: 4 moles*30 g/mol= 120 g
  • H₂O: 6 moles*18 g/mol= 108 g

Now to calculate the necessary mass of O₂ for a complete reaction, the rule of three is applied as follows: if by stoichiometry 68 g of NH₃ react with 160 g of O₂, 7.5 g of NH₃ with how many grams of O₂ will it react?

mass of O_{2} =\frac{7.5 g of NH_{3} * 160 g of O_{2} }{68 g of NH_{3} }

mass of O₂≅17.65 g

<u><em>17.65 grams of O2 are needed for a complete reaction.</em></u>

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Answer:

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The bond is not symmetrical to the internuclear axis and on rotation the axis, the bond breaks.

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