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ipn [44]
3 years ago
15

How do nonnumeric, or conceptual problems, differ from numeric problems

Chemistry
2 answers:
Andru [333]3 years ago
5 0
<span>Nonnumeric, or conceptual problems, differ from numeric problems in a sense that solutions to conceptual problems do not involve or need calculations. It just need your knowledge on that specific subject and you just have to analyze the question and understand it to answer correctly.</span>
Sladkaya [172]3 years ago
4 0

Answer:

Answered

Explanation:

Non numeric problems are designed only test the conceptual clarity of the pupil without going into details of calculations. Generally, conceptual problems are asked to check the basic understanding of the topic or the subject

Whereas numerical problem are asked to check whether the student is able to apply the concept or not, through some real world data.

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If 42.9 mL of rubbing alcohol is
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Answer:

19.8 %

Explanation:

V% = ( V of solute \ 100 ml  of solution ) ×100%  =

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3 years ago
Using the table provided, which of the following answer choices has the largest entropy?
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3 years ago
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Calculate the amount of heat released when 27.0 g H2O is cooled from a liquid at 314 K to a solid at 263 K. The melting point of
BlackZzzverrR [31]

Answer : The amount of heat released, 45.89 KJ

Solution :

Process involved in the calculation of heat released :

(1):H_2O(l)(314K)\rightarrow H_2O(l)(273K)\\\\(2):H_2O(l)(273K)\rightarrow H_2O(s)(273K)\\\\(3):H_2O(s)(273K)\rightarrow H_2O(s)(263K)

Now we have to calculate the amount of heat released.

Q=[m\times c_{p,l}\times (T_{final}-T_{initial})]+\Delta H_{fusion}+[m\times c_{p,s}\times (T_{final}-T_{initial})]

where,

Q = amount of heat released = ?

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c_{p,l} = specific heat of liquid water = 4.184 J/gk

c_{p,s} = specific heat of solid water = 2.093 J/gk

\Delta H_{fusion} = enthalpy change for fusion = 40.7 KJ/mole = 40700 J/mole

conversion : 0^oC=273k

Now put all the given values in the above expression, we get

Q=[27g\times 4.184J/gK\times (314-273)k]+40700J+[27g\times 2.093J/gK\times (273-263)k]

Q=45896.798J=45.89KJ     (1 KJ = 1000 J)

Therefore, the amount of heat released, 45.89 KJ

7 0
3 years ago
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A student uses a calorimeter to determine the enthalpy of dissolving for ammonium nitrate. The student fills a calorimeter with
ale4655 [162]
Enthalpy change during the dissolution process = m c ΔT,

here, m = total mass = 475 + 125 = 600 g
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<span>
Therefore, </span>Enthalpy change during the dissolution = 600 x 4.18 X (-16.2)
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Thus, <span>enthalpy of dissolving of the ammonium nitrate is -40630 J/g</span>

7 0
3 years ago
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