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3 years ago

Rank the solutions below in order of increasing acidity. (Drag and drop into the appropriate area)

Chemistry

1 answer:

Vladimir79 [104]3 years ago

7 0

Answer:

0.1 M NaOH, 3 M NH3, 0.01 M CH3COOH, 0.01 M H2SO4, 0.1 M HCl

Explanation:

Strong acids are more acids than weak acids. In the same way, strong bases are more basic than weak bases that are in the same concentration.

Then, the more concentrated acid or base will be more acidic or basic.

CH3COOH. Weak acid

NaOH. Strong base

H2SO4. Strong acid

NH3. Weak base.

HCl. Strong acid

The less acid (More basic):

Strong base, weak base, weak acid, diluted strong acid, undiluted strong acid

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The movement of tectonic plates is so slow and gradual that you cannot see or feel them moving. As a result, scientist depend on

guapka [62]

Answer:

centimeters per year

Explanation:

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2 years ago

What are some examples of gases at room temperature

Lady_Fox [76]

Answer:

Nitrogen, Hydrogen, Oxygen, Chlorine, and Fluorine are all gases at room temperature.

Explanation:

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2 years ago

Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°

Pavel [41]

Answer:

PNO₂ = 0.49 atm

PN₂O₄ = 0.45 atm

Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that involves the density (ρ = m/V).

PV = nRT

n = m/M (m is the mass, and M the molar mass)

$PV = \frac{m}{M}RT$

$PxM = \frac{m}{V}RT$

PxM = ρRT

ρ = PxM/RT

With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

$2.7 = \frac{0.94xMavg}{0.082x289}$

0.94Mavg = 63.9846

Mavg = 68.0687 g/mol

The molar mass of N is 14 g/mol and of O is 16 g/mol, than $M_{NO2} = 46$ g/mol and $M_{N2O4} = 96$ g/mol. Calling y the molar fraction:

$Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}$

And,

$y_{NO2} + y_{N2O4} = 1$

$y_{N2O4} = 1 - y_{NO2}$

So,

$68.0687 = 46y_{NO2} + 92x(1 - y_{NO2})$

$68.0687 - 92 = 46y_{NO2} - 92y_{NO2}$

$46y_{NO2} = 23.9313$

$y_{NO2} = 0.52$

$y_{N2O4} = 0.48$

The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

8 0

3 years ago

2KClO3(s) => 2KCl(s) + 3O2(g) <br> is there an increase or decrease of entropy?

ValentinkaMS [17]

Answer:

Entropy increases

Explanation:

Entropy (S) is a measure of the degree of disorder. For a given substance - say water - across phases the following is true ...

S(ice) < S(water) << S(steam)

For a chemical process, entropy changes can be related to increasing or decreasing molar volumes of gas from reactant side of equation to product side of equation. That is ...

if molar volumes of gas increase, then entropy increases, and

if molar volumes of gas decrease, then entropy decreases.

For the reaction 2KClO₃(s) => 2KCl(s) + 3O₂(g)

molar volumes of gas => 0Vm* 0Vm 3Vm

*molar volumes (Vm) apply only to gas phase substances. Solids and liquids do not have molar volume.

Since the reaction produces 3 molar volumes of O₂(g) product vs 0 molar volumes of reactant, then the reaction is showing an increase in molar volumes of gas phase substances and its entropy is therefore increasing.

3 0

3 years ago

Identify ALL the possible mol ratio from<br> this balanced equation:

grandymaker [24]

Answer:

$\frac{1 mole of N_{2} }{3 moles of H_{2} }$

Explanation:

The equation of the reaction:

Nitrogen gas N₂ reacts with Hydrogen as H₂ to produce ammonia NH₃;

N₂ + H₂ → NH₃

The balanced equation is ;

N₂ + 3H₂ → 2NH₃

The mole ratio is the ratio of the coefficients of the combining reactants;

1 mole of N₂ combines with 3 mole of H₂;

So;

$\frac{1 mole of N_{2} }{3 moles of H_{2} }$

3 0

2 years ago