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VladimirAG [237]
3 years ago
5

If 8.700 g of c6h6 is burned and the heat produced from the burning is added to 5691 g of water at 21 °c, what is the final tem

perature of the water?
Chemistry
1 answer:
leonid [27]3 years ago
8 0
C₆H₆ is benzene which has a molar mass of 78 g/mol. When benzene is burned, the reaction is called combustion. The heat produced in this reaction is called the heat of combustion. For benzene, the heat of combustion is -3271 kJ/mol.

Heat of benzene = (8.7 g)(1 mol/78 g)(-3271 kJ/mol) = -364.84 kJ

By conservation of energy,
Heat of benzene = - Heat of water
where
Heat of Water = mCp(Tf - T₀)
where Cp for water is 4.187 kJ/kg·°C

Thus,

-364.84 kJ = -(5691 g)(1 kg/1000 g)(4.187 kJ/kg·°C)(Tf - 21)
<em>Tf = 36.31°C</em>
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Your teacher directs you to combine two liquid substances into a flask. after you combine them, you notice that the flask feels
adelina 88 [10]

Answer : The correct option is (A).

Explanation :

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3 0
3 years ago
How many grams of ethanol c2h5oh can be made by the fermentation of 1150 g of glucose?
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Answer is: 588.15 <span>grams of ethanol.
</span>Chemical reaction: C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂.
m(C₆H₁₂O₆) = 1150 g.
n(C₆H₁₂O₆) = m(C₆H₁₂O₆) ÷ M(C₆H₁₂O₆).
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n(C₆H₁₂O₆) = 6.38 mol.
From chemical reaction: n(C₆H₁₂O₆) : n(C₂H₅OH) = 1 : 2.
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5 0
3 years ago
Boron trifluoride gas is collected at 2.0 degree C in an evacuated flask with a measured volume of 15.0 L. When all the gas has
IgorC [24]

Answer:

Moles of boron trifluoride gas that were collected = 11.6 mol

Mass of boron trifluoride gas that were collected = 787 g

Explanation:

Given that:

Temperature = 2.0 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (2.0 + 273.15) K = 275.15 K

V = 15.0 L

Pressure = 0.130 atm

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L atm/ K mol  

Applying the equation as:

0.130 atm × 15.0 L = n ×0.0821 L atm/ K mol  × 275.15 K

⇒n = 11.6 mol

<u>Thus, Moles of boron trifluoride gas that were collected = 11.6 mol </u>

Molar mass of boron trifluoride gas = 67.82 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

11.6\ mole= \frac{Mass}{67.82\ g/mol}

<u>Mass of boron trifluoride gas that were collected = 787 g</u>

7 0
2 years ago
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