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3 years ago

Please answer as soon as possible if you can

Chemistry

1 answer:

alexgriva [62]3 years ago

5 0

Answer:

Second one

Explanation:

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An unknown amount of sodium azide (NaN3) reacts and produces 0.033 moles of nitrogen gas. What mass of sodium metal is produced

Monica [59]

Answer:

Mass of sodium metal is 130.87 gram

Explanation:

The complete reaction is

2 NaN3 --> 2 Na + 3 N2

We know that PV = nRT

n = $\frac{PV}{RT}$

On substituting the given values, we get

$n = \frac{\frac{99707}{101325}*75 }{0.082 *(273.15 +15)} \\n = 3.02$ moles of N2

Sodium azide's molar mass

3.02 *(2/3) = 2.013 moles

Mass = 2.03 * 65.01 = 130.87 gram

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3 years ago

HELPPP simply the expression!!!!

coldgirl [10]

Answer:

$\frac{3}{ \sqrt{3} } \times \frac{ \sqrt{3} }{ \sqrt{3} } = \frac{3 \sqrt{3} }{3} = \sqrt{3}$

when there is a radical in the denominator, we should rationalize (mutiply the denominator and numerator by the radical) to get rid of the radical in the denominator.

4 0

2 years ago

What molecule is removed during dehydration synthesis?.

nignag [31]

Answer: two hydrogen atoms and one oxygen atom are removed during dehydration synthesis.

Hope this helps!

4 0

2 years ago

The equilibrium 2NO(g)+Cl2(g)⇌2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures

QveST [7]

Answer:

For A: The $K_p$ for the given reaction is $4.0\times 10^1$

For B: The $K_c$ for the given reaction is 1642.

Explanation:

The given chemical reaction follows:

$2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)$

For A:

The expression of $K_p$ for the above reaction follows:

$K_p=\frac{(p_{NOCl})^2}{(p_{NO})^2\times p_{Cl_2}}$

We are given:

$p_{NOCl}=0.24 atm\\p_{NO}=9.10\times 10^{-2}atm=0.0910atm\\p_{Cl_2}=0.174atm$

Putting values in above equation, we get:

$K_p=\frac{(0.24)^2}{(0.0910)^2\times 0.174}\\\\K_p=4.0\times 10^1$

Hence, the $K_p$ for the given reaction is $4.0\times 10^1$

For B:

Relation of $K_p$ with $K_c$ is given by the formula:

$K_p=K_c(RT)^{\Delta ng}$

where,

$K_p$ = equilibrium constant in terms of partial pressure = $4.0\times 10^1$

$K_c$ = equilibrium constant in terms of concentration = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature = 500 K

$\Delta ng$ = change in number of moles of gas particles = $n_{products}-n_{reactants}=2-3=-1$

Putting values in above equation, we get:

$4.0\times 10^1=K_c\times (0.0821\times 500)^{-1}\\\\K_c=\frac{4.0\times 10^1}{(0.0821\times 500)^{-1})}=1642$

Hence, the $K_c$ for the given reaction is 1642.

7 0

3 years ago

A student mixes 20.0gof white KCl crystals with distilled water in a beaker. After the mixture was stirred, no crystals are visi

mixas84 [53]

Answer:d

Explanation: over time water evaporates which leaves you with the white crystals mass

6 0

2 years ago