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3 years ago

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1 answer:

zhenek [66]3 years ago

6 0

Answer:

Air pollution

Explanation:

Carbon(IV)oxide is sometimes harmful to man but good for plant in other to manufacture their food

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Which of the following best explains the relationship between molecules and atoms?

mr Goodwill [35]

The answer is A sorry if I didn’t explain but it’s A

8 0

3 years ago

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What is the name of the compound with the formula crso4?

ludmilkaskok [199]

<span>Chromium(II) sulfate

this is an ionic compound of a metal and a polyatomic ion.
chromium is a metal that can form more than one type of cation. In this case, the polyatomic ion name is sulfate and it has 2 negative charges. Then Cr has to have 2 positive charges.

then write the name of the metal followed by the charge of the ion between parenthesis and in roman numbers followed by the name of the polyatomic ion.</span>

3 0

4 years ago

What is the heat of vaporization of ethanol, given that ethanol has a normal boiling point of 63.5°C and the vapor pressure of e

Serjik [45]

Explanation:

According to Clausius-Claperyon equation,

$ln (\frac{P_{2}}{P_{1}}) = \frac{-\text{heat of vaporization}}{R} \times [\frac{1}{T_{2}} - \frac{1}{T_{1}}]$

The given data is as follows.

$T_{1} = 63.5^{o}C$ = (63.5 + 273) K

= 336.6 K

$T_{2} = 78^{o}C$ = (78 + 273) K

= 351 K

$P_{1}$ = 1 atm, $P_{2}$ = ?

Putting the given values into the above equation as follows.

$ln (\frac{P_{2}}{P_{1}}) = \frac{-\text{heat of vaporization}}{R} \times [\frac{1}{T_{2}} - \frac{1}{T_{1}}]$

$ln (\frac{1.75 atm}{1 atm}) = \frac{-\text{heat of vaporization}}{8.314 J/mol K} \times [\frac{1}{351 K} - \frac{1}{336.6 K}]$

$\Delta H$ = $\frac{0.559}{1.466 \times 10^{-4}} J/mol$

= $0.38131 \times 10^{4} J/mol$

= 3813.1 J/mol

Thus, we can conclude that the heat of vaporization of ethanol is 3813.1 J/mol.

4 0

3 years ago

How many grams are in 36.2 moles of Iron (I) fluoride?

Allushta [10]

Answer:

4084.808 grams (SigFigs: 4085 grams)

Explanation:

The molar mass of Iron fluoride is 112.84 g/mol.

To calculate the mass, multiply the molar mass by the number of moles.

36.2 mol * 112.84 g/mol = 4084.808 g

Convert to Sigfigs (if necessary):

4085 g

5 0

3 years ago

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"The combustion of ethylene proceeds by the reaction C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) When the rate of disappearance of O2 i

Julli [10]

Answer:

The rate of disappearance of $C_2H_4$ is 0.0766 M/s.

Explanation:

$C_2H_4(g)+3O_2(g)\rightarrow 2CO_2(g)+2H_2O(g)$

Rate of the reaction = R

$R=-\frac{1}{1}\frac{d[C_2H_4]}{dt}=-\frac{1}{3}\frac{d[O_2]}{dt}$

[te]R=\frac{1}{2}\frac{d[CO_2]}{dt}=\frac{1}{2}\frac{d[H_2O]}{dt}[/tex]

Rate of disappearance of $O_2$ =0.23 M/s

Rate of disappearance of $O_2=3\times R$

$0.23 M/s=3\times R$

R =0.07666 M/s

Rate of disappearance of $C_2H_4=1\times R$

$\frac{d[C_2H_4]}{dt}=1\times 0.23 m/s=0.0766 M/s$

The rate of disappearance of $C_2H_4$ is 0.0766 M/s.

7 0

4 years ago