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LekaFEV [45]
3 years ago
6

Consider the reaction 2 NO + O2 → 2 NO2

Chemistry
1 answer:
Sonbull [250]3 years ago
5 0

Answer:

(a) Rate at which NO_2 is formed is 0.050 M/s

(b) Rate at which O_2 is consumed is 0.0250 M/s.

Explanation:

The given reaction is:-

2NO+O_2\rightarrow 2NO_2

The expression for rate can be written as:-

-\frac{1}{2}\frac{d[NO]}{dt}=-\frac{d[O_2]}{dt}=\frac{1}{2}\frac{d[NO_2]}{dt}

Given that:- \frac{d[NO]}{dt}=-0.050\ M/s (Negative sign shows consumption)

-\frac{1}{2}\frac{d[NO]}{dt}=\frac{1}{2}\frac{d[NO_2]}{dt}

-\frac{d[NO]}{dt}=\frac{d[NO_2]}{dt}

-(-0.050\ M/s)=\frac{d[NO_2]}{dt}

\frac{d[NO_2]}{dt}=0.050\ M/s

(a) Rate at which NO_2 is formed is 0.050 M/s

-\frac{1}{2}\frac{d[NO]}{dt}=-\frac{d[O_2]}{dt}

-\frac{1}{2}\times -0.050\ M/s=-\frac{d[O_2]}{dt}

\frac{d[O_2]}{dt}=0.0250\ M/s

(b) Rate at which O_2 is consumed is 0.0250 M/s.

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When 0.514 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 C to 29.4 C. Find ⌂E rxn for the combustion of biphenyl in kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/ C. 



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3 0
3 years ago
Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO
stiv31 [10]

Answer:

NO would form 65.7 g.

H₂O would form 59.13 g.

Explanation:

Given data:

Moles of NH₃ = 2.19

Moles of O₂ = 4.93

Mass of NO produced = ?

Mass of  produced H₂O = ?

Solution:

First of all we will write the balance chemical equation,

4NH₃ + 5O₂   →   4NO + 6H₂O

Now we will compare the moles of NO and H₂O with ammonia from balanced chemical equation:

NH₃  :   NO                                   NH₃  :   H₂O

4     :    4                                          4    :      6

2.19   :    2.19                                 2.19  : 6/4 × 2.19 = 3.285 mol

Now we will compare the moles of NO and H₂O with oxygen from balanced chemical equation:

O₂  :   NO                                               O₂ :   H₂O

5     :    4                                                  5     :    6

4.93   :   4/5×4.93 = 3.944 mol               4.93  : 6/5 × 4.93 = 5.916 mol

we can see that moles of water and nitrogen monoxide produced from the ammonia are less, so ammonia will be limiting reactant and will limit the product yield.

Mass of water = number of  moles × molar mass

Mass of water = 3.285 mol × 18 g/mol

Mass of water = 59.13 g

Mass of nitrogen monoxide  = number of  moles × molar mass

Mass of nitrogen monoxide = 2.19 mol × 30 g/mol

Mass of nitrogen monoxide = 65.7 g

4 0
3 years ago
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Answer:

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Answer:

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Explanation:

4 0
3 years ago
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