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3 years ago

13

The tank of an air compressor contains gas at normal atmospheric pressure (1atm). If the compressor motor pumps the equivalent o

f three extra tanks of air into the compressor tank, what will be the final pressure

1 answer:

Eduardwww [97]3 years ago

4 0

Answer:

4atm

Explanation:

1atm+3Atm

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How many grams of aluminum will<br> react fully with 1.25 moles Cl₂?

Liula [17]

2Al + 3Cl₂ → 2AlCl₃

mol Al = 2/3 x 1.25 = 0.83

mass Al = 0.83 x 27 g/mol = 22.41 g

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3 years ago

What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 11.0 L of water to produce an antifreeze solution wi

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Answer:

The volume of ethylene glycol, we must add is 8.2 L

Explanation:

Let's apply the formula for the colligative property of Depression of freezing point, to solve this

ΔT = Kf . m . i

Where ΔT = Fussion T° in pure solvent - Fussion T° in solution

Kf = Cryoscopic constant (equal to 1.86 °C kg/mol for the freezing point of water)

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i = The number of ions dissolved in solution. As it is a non-electrolytic compound, the i values 1 (Van't Hoff factor)

0°C - (-25°C) = 1.86 kg°C/mol . m

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13.4 = mol/kg

As water density is 1 g/ml, let's convert firstly 11L in mL

11L .1000 = 11000mL

In conclusion, we have 11000 g of water.

density = mass / volume

So, if we have 13.4 moles in 1 kg of water, how many moles of ethylene glycol do we have, in 11000 g of water.

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Now we can apply density of ethylene glycol to find out the volume

Density ethylene glycol = ethylene glycol mass / ethylene glycol volume

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ethylene glycol volume = 9149.1 g/ 1.11 g/ml

ethylene glycol volume = 8242 mL

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4 years ago

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Galina-37 [17]

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Explanation:

To calculate the number of moles for given molarity, we use the equation:

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a) $\text{Moles of carbonate}=\frac{0.2moldm^{-3}\times 25cm^3}{1000}=0.005mol$

b) $\text{Moles of acid}=\frac{0.5moldm^{-3}\times 20cm^3}{1000}=0.01mol$

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3 years ago

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4 years ago

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Answer:

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