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vova2212 [387]
3 years ago
6

(3 points)

Chemistry
2 answers:
Paul [167]3 years ago
5 0
An increased number of rod cells
Black_prince [1.1K]3 years ago
4 0
The answer is A I did this question before it’s A
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Humans opinions of evolution.
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What best defines an extensive property of a substance? (4 points) A property that is observable A property that is measurable A
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A physical property that depends on the sample size 

Explanation:

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The following thermochemical equation is for the reaction of nitrogen(g) with oxygen(g) to form nitrogen dioxide(g). N2(g) + 2O2
Rzqust [24]

<u>Answer:</u> The mass of nitrogen gas reacted to produce given amount of energy is 5.99 grams.

<u>Explanation:</u>

The given chemical reaction follows:

N_2(g)+2O_2(g)\rightarrow 2NO_2(g);\Delta H=66.4kJ

We know that:

Molar mass of nitrogen gas = 28 g/mol

We are given:

Enthalpy change of the reaction = 14.2 kJ

To calculate the mass of nitrogen gas reacted, we use unitary method:

When enthalpy change of the reaction is 66.4 kJ, the mass of nitrogen gas reacted is 28 grams.

So, when enthalpy change of the reaction is 14.2 kJ, the mass of nitrogen gas reacted will be = \frac{28}{66.4}\times 14.2=5.99g

Hence, the mass of nitrogen gas reacted to produce given amount of energy is 5.99 grams.

8 0
3 years ago
Tetrachloromethane, CCl4 is produced from the substitution reaction between methane and chlorine gas. If the rate of formation o
Korolek [52]

The rate of disappearance of chlorine gas : 0.2 mol/dm³

<h3>Further explanation</h3>

The reaction rate (v) shows the change in the concentration of the substance (changes in addition to concentrations for reaction products or changes in concentration reduction for reactants) per unit time.

For reaction :

\tt aA+bB\rightarrow cC+dD

The rate reaction :

\tt -\dfrac{1}{a}\dfrac{d[-A]}{dt}= -\dfrac{1}{b}\dfrac{d[-B]}{dt}=\dfrac{1}{c}\dfrac{d[C]}{dt}=\dfrac{1}{d}\dfrac{d[D]}{dt}

Reaction for formation CCl₄ :

<em>CH₄+4Cl₂⇒CCl₄+4HCl</em>

<em />

From equation, rate of reaction = rate of formation CCl₄ = 0.05 mol/dm³

Rate of formation of  CCl₄  = reaction rate x coefficient of  CCCl₄

0.05 mol/dm³ = reaction rate x 1⇒reaction rate = 0.05 mol/dm³

The rate of disappearance of chlorine gas (Cl₂) :

Rate of disappearance of  Cl₂  = reaction rate x coefficient of  Cl₂

Rate of disappearance of  Cl₂ = 0.05 x 4 = 0.2 mol/dm³

4 0
3 years ago
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