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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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<h3>Answer:</h3>

70.906 g

<h3>Explanation:</h3>

We are given;

  • Atoms of Chlorine = 1.2 × 10^24 atoms

We are required to calculate the mass of Chlorine

  • We know that 1 mole of an element contains atoms equivalent to the Avogadro's number, 6.022 × 10^23.
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But since Chlorine gas is a molecule;

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But, molar mass of Chlorine gas = 70.906 g/mol

Then;

70.906 g Of chlorine gas = 2 × 6.022 × 10^23 atoms

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Thus;

For 1.2 × 10^24 atoms ;

= ( 70.906 g/mol × 1.2 × 10^24 atoms ) ÷ (1.20 × 10^24 atoms)

<h3>=  70.906 g </h3>

Therefore, 1.20 × 10^24 atoms of chlorine contains a mass of 70.906 g

=  

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