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2 years ago

I WILL MARK Brainest

Chemistry

1 answer:

wolverine [178]2 years ago

5 0

It should be sketch,identify, dig, then set water for the watering times, hope this helps, hope you feel better soon

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A 0.327-g sample of azulene (C10H8) is burned in a bomb calorimeter and the temperature increases from 25.20 °C to 27.60 °C. The

liq [111]

Explanation:

The given data is as follows.

Molecular weight of azulene = 128 g/mol

Hence, calculate the number of moles as follows.

No. of moles = $\frac{mass}{\text{molecular weight}}$

= $\frac{0.392 g}{128 g/mol}$

= 0.0030625 mol of azulene

Also, $-Q_{rxn} = Q_{solution} + Q_{cal}$

$Q_{rxn} = n \times dE$

$Q_{solution} = m \times C \times (T_{f} - T_{i})$

$Q_{cal} = C_{cal} \times (T_{f} - T_{i})$

Now, putting the given values as follows.

$Q_{solution} = 1.17 \times 10^{3} g \times 10^{3} \times 4.184 J/g^{o}C \times (27.60 - 25.20)^{o}C$

= 11748.67 J

So, $Q_{cal} = 786 J/^{o}C \times (27.60 - 25.20)^{o}C$

= 1886.4 J

Therefore, heat of reaction will be calculated as follows.

$-Q_{rxn}$ = (11748.67 + 1886.4) J

= 13635.07 J

As, $Q_{rxn} = n \times dE$

13635.07 J = $-n \times dE$

dE = $\frac{13635.07 J}{0.0030625 mol}$

= 4452267.75 J/mol

or, = 4452.26 kJ/mol (as 1 kJ = 1000 J)

Thus, we can conclude that $\Delta E$ for the given combustion reaction per mole of azulene burned is 4452.26 kJ/mol.

7 0

3 years ago

Vitamin A information please with detail

avanturin [10]

Vitamin A is an essential vitamin that the body needs for growth and development. It is also vital for cell recognition, vision, immune function, and reproduction.

It also helps the heart, lungs, kidneys, and other organs function correctly.

Vitamin A deficiency is rare in the United States. If it happens, it can lead to eye problems, including night blindness.

In this article, learn more about the types of vitamin A, what vitamin A does, and some good sources of it.

5 0

2 years ago

4) The Maunder Minimum would include which of the following years? A. 1855 - 1900 B. 1910 - 1930 C. 1979 - 1987 D. 1670 - 1700 S

ivolga24 [154]

The answer is B
have a nice day.....

4 0

3 years ago

Calculate the density of CO2 in g/cm3 at room temperature(25 degrees Celsuis) and pressure(1 atm) assuming it acts as an ideal g

Readme [11.4K]

Answer:

$density=1.8x10^{-3}g/mL$

Explanation:

Hello,

Considering the ideal equation of state:

$PV=nRT$

The moles are defined in terms of mass as follows:

$n=\frac{m}{M}$

Whereas $M$ the gas' molar mass, thus:

$PV=\frac{mRT}{M}$

Now, since the density is defined as the quotient between the mass and the volume, we get:

$P=\frac{m}{V} \frac{RT}{M}$

Solving for $m/V$ :

$density= m/V=\frac{PM}{RT}$

Thus, the result is given by:

$density=\frac{(1atm)(44g/mol)}{[0.082atm*L/(mol*K)]*298.15K} \\density=1.8g/L=1.8x10^{-3}g/mL$

Best regards.

8 0

3 years ago

Will mark as Brainliest.

LUCKY_DIMON [66]

Gas i took the test plz mark brainliest!

8 0

3 years ago

Read 2 more answers