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allochka39001 [22]
3 years ago
15

PLEASE HELP ME 20 POINTS!!!!!

Chemistry
1 answer:
julsineya [31]3 years ago
5 0

Answer:

Theoretical yield of the reaction is 121·38 g

The excess reactant is hydrogen

The limiting reactant is nitrogen

Explanation:

By assuming that the reaction between nitrogen and hydrogen taking place in presence of catalyst because at normal conditions the reaction between them will not occur

Number of moles of nitrogen taken are 100÷28 ≈ 3.57

Number of moles of hydrogen taken are 100÷2 = 50

Actually the reaction between nitrogen and hydrogen takes place according to the following equation

<h3>Nx_{2} + 3Hx_{2}  → 2NHx_{3}</h3>

So from the equation for 1  mole of nitrogen and 3 moles of hydrogen we get 2 moles of ammonia

Here in the problem we have approximately 3·57 moles of nitrogen so we require 3×3·57 moles of hydrogen

∴ Number of moles of hydrogen required is 10·71

But we have 50 moles of hydrogen

∴ Excess reagent is hydrogen and limiting reagent is nitrogen

Number of moles of ammonia produced  is 2×3·57 = 7·14

Weight of ammonia is 17 g

∴ Amount of ammonia produced is 17×7·14 = 121·38 g

∴ Theoretical yield of the reaction is 121·38 g

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The specific heat capacity, C, of the substance is 3.94 \frac{J}{g-^oC}. To raise one gram of a substance by one degree Celsius, a specific amount of heat must be absorbed. This is called the specific heat of the substance. The higher the specific heat of a substance, the more energy is needed to increase its temperature and vice versa.

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The specific heat capacity, C, of a substance is related to the amount of substance and the temperature change using the following equation

q \ = \ mC(T_{f}-T_{i})

where

q = amount of heat absorbed (usually in J)

m = amount of substance (in g)

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To answer the problem, we sort the given information:

q = 22974 J (5 significan figures)

m = 96.5 g (3 significant figures)

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T(i) = 13.46 °C (4 significant figures)

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C \ = \frac{q}{m(T_{f} \ - \ T_{i})}

Plug in the values to the equation above to get the value of C.

C \ = \ \frac{22974 \ J}{96.5 \ g \ (73.86 \ \ -13.46 \°C)} \\C \ = \ \frac{22974 \ J}{96.5 \ g \ (60.4\°C)} \\C \ = \ \frac{22974 \ J}{5828.6 \ g -\°C} \\C \ = \ 3.941598 \ \frac{J}{g -\°C} \\

Since the least number of significant figures in the given is 3, then the final answer must have 3 significant figures, too. Therefore,

\boxed {C = 3.94 \ \frac{J}{ g -\°C}}

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<u>Learn More: </u>

1. Learn more about heat capacity brainly.com/question/8828503

2. Learn more about calorimetry brainly.com/question/8168263

3. Learn more about heat of reaction brainly.com/question/10122365

<u>Keywords:</u> heat capacity, specific heat, calorimetry

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