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3 years ago

12

Name the gas liberated when ethanol react with sodium metal?

1 answer:

expeople1 [14]3 years ago

4 0

<span>When sodium reacts with ethanol, hydrogen gas liberates and leaves a colorless solution of Alkoxide

Reaction: 2CH</span>₃CH₂OH + 2Na → 2CH₃CH₂ONa + H₂

So, in short the answer of your particular question will be "Hydrogen Gas"

Hope this helps!!!

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What is the pH of a bleach solution that has a [OH−]=1.3×10−4 M?

Delvig [45]

Answer:

pH = 10.113

Explanation:

Here, we can find pOH first:

pOH = $-log([OH^-])$ = 3.886.

Then, we can find pH which is 14 - pOH. We then get the answer above.

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3 years ago

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djverab [1.8K]

Answer:

P₂ = 394.4 KPa

Explanation:

Given data:

Volume of gas = 152 dm³

Pressure of gas = 98.6 KPa

Final pressure = ?

Final volume = quartered = 1/4×152 = 38 dm³

Solution:

P₁V₁ = P₂V₂

P₂ = P₁V₁/V₂

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3 years ago

Consider the following reaction:

Kitty [74]

Answer : The value of equilibrium constant (Kc) is, 0.0154

Explanation :

The given chemical reaction is:

$SO_2Cl_2(g)\rightarrow SO_2(g)+Cl_2(g)$

Initial conc. $2.4\times 10^{-2}$ 0 0

At eqm. $(2.4\times 10^{-2}-x)$ x x

As we are given:

Concentration of $Cl_2$ at equilibrium = $1.3\times 10^{-2}M$

That means,

$x=1.3\times 10^{-2}M$

The expression for equilibrium constant is:

$K_c=\frac{[SO_2][Cl_2]}{[SO_2Cl_2]}$

Now put all the given values in this expression, we get:

$K_c=\frac{(x)\times (x)}{2.4\times 10^{-2}-x}$

$K_c=\frac{(1.3\times 10^{-2})\times (1.3\times 10^{-2})}{2.4\times 10^{-2}-1.3\times 10^{-2}}$

$K_c=0.0154$

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3 years ago

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The atomic mass is the average of the isotopes of the element meaning most averages of isotopes will not be whole numbers

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