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3 years ago

Calculate the mass of aluminum bromide that can be produced from 4.4 mil of bromide

Chemistry

1 answer:

Aloiza [94]3 years ago

7 0

Answer:

197 grams

Explanation:

Without taking into account the number of sig figs you have for your values, you can say that the answer will once again be

197 g of aluminium bromide.

(I hope this is right)

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A monoprotic weak acid, HA , dissociates in water according to the reaction:

Ratling [72]

<u>Answer:</u> The $pKa$ of the acid is 6.09

<u>Explanation:</u>

For the given chemical reaction:

$HA(aq.)\rightleftharpoons H^+(aq.)+A^-(aq.)$

The expression of equilibrium constant [tex[(K_a)[/tex] for the above equation follows:

$K_a=\frac{[H^+][A^-]}{[HA]}$

We are given:

$[HA]_{eq}=0.200M$

$[H^+]_{eq}=4.00\times 10^{-4}M$

$[A^-]_{eq}=4.00\times 10^{-4}M$

Putting values in above expression, we get:

$K_a=\frac{(4.00\times 10^{-4})\times (4.00\times 10^{-4}}{0.200}\\\\K_a=8.0\times 10^{-7}0$

p-function is defined as the negative logarithm of any concentration.

$pKa=-\log(K_a)$

So,

$pKa=-\log(8.0\times 10^{-7})\\\\pKa=6.09$

Hence, the $pKa$ of the acid is 6.09

7 0

3 years ago

A mixture contains two or more substances chemically combined while a compound contains two or more substances physically combin

Alex73 [517]

True I'm pretty sure

6 0

3 years ago

2 Students were asked to identify the location of elements in the periodic table based on clues

rjkz [21]

Answer:

Explanation:

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3 years ago

The freezing point of water H2O is 0.00°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in water is urea. If 13.

Trava [24]

Answer:

Molality = 1.46 molal

The freezing point of the solution = -2.72 °C

Explanation:

Step 1: Data given

The freezing point of water H2O is 0.00°C at 1 atmosphere

urea = nonelectrolyte = van't Hoff factor = 1

Mass urea = 13.40 grams

Molar mass urea = 60.1 g/mol

Mass of water = 153.2 grams

Molar mass H2O = 18.02 g/mol

Kf = 1.86 °C/m

Step 2: Calculate moles urea

Moles urea = mass urea /molar mass urea

Moles urea = 13.40 grams / 60.1 g/mol

Moles urea = 0.223 moles

Step 3: Calculate the molality

Molality = moles urea / mass water

Molality = 0.223 moles / 0.1532 kg

Molality = 1.46 molal

Step 4: Calculate the freezing point of the solution

ΔT = i * Kf * m

ΔT = 1* 1.86 °C/m * 1.46 m

ΔT = 2.72 °C

The freezing point = -2.72 °C

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3 years ago

What makes carbon monoxide

Leto [7]

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3 years ago

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