A solution that is at equilibrium must be(1) concentrated (3) saturated(2) dilute (4) unsaturated

Answers

Answer 1

Answer:

Answer:

(3) saturated

Explanation:

Hello,

In this case, a solution that is at equilibrium must be (3) saturated as at the equilibrium, the entire solute is completely dissolved into the solvent, so no leftovers are present. Unsaturated solutions are not at equilibrium since there is a portion of solvent that is not contributing to equilibrium. Concentrated solutions are not at equilibrium since they could have more solution than allowed into the solvent.

Best regards.

Answer 2

Answer: A solution that is at equilibrium must be saturated.

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Which statement describes a chemical property of aluminum?(1) Aluminum is malleable.
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Answers

The correct answer as to which statement describes a chemical property of aluminum would be that it reacts with sulfuric acid.

There are two properties of every substance - physical and chemical properties.

Physical properties refer to the characteristics that can be observed without altering the substance while chemical properties refer to the characteristics of undergoing chemical changes in reactions.

Physical properties include color, boiling and melting point, hardness etc., while chemical properties include reactivity, toxicity, flammability, etc.

All the options have to do with physical properties of aluminum except its reactivity with sulfuric acid. The equation of reaction is as follows:

Al + H2SO4 ---> Al2(SO4)3 + H2

More on the chemical properties of aluminum can be found here: brainly.com/question/536562

Aluminium reacts with sulphuric acid.

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What is the percent composition by mass of nitrogen in (NH4)2CO3 (gram-formula mass = 96.0 g/mol)? (1) 14.6%
(2) 29.2%
(3) 58.4%
(4) 87.5%

Answers

The percentage composition by mass of nitrogen in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is $\boxed{\left( 2 \right){\text{ 29}}{\text{.2 \% }}}$ .

Further explanation:

The most commonly applied concentration terms are as follows:

1. Molality

2. Mole fraction

3. Molarity

4. Parts per million

5. Mass percent

6. Volume percent

7. Percentage composition

The given compound is ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ . It contains two atoms of nitrogen, eight atoms of hydrogen, one atom of carbon and three atoms of oxygen.

The mass of nitrogen in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ can be calculated as follows:

${\text{Mass of N}} =\left( {{\text{Number of nitrogen atoms}}} \right)\left( {{\text{Molar mass of nitrogen}}} \right)$ …… (1)

The number of N atoms in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is 2.

The molar mass of nitrogen is 14.01 g/mol.

Substitute these values in equation (1).

$\begin{aligned}{\text{Mass of nitrogen}} &= \left( {\text{2}} \right)\left( {{\text{14}}{\text{.01 g/mol}}} \right)\n&= 28.02{\text{ g/mol}}\n\end{aligned}$

The formula to calculate the percentage composition of N in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is as follows:

${\text{\% composition of N}} = \left( {\frac{{{\text{Mass of N}}}}{{{\text{Mass of }}{{\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)}_{\text{2}}}{\text{C}{{\text{O}}_{\text{3}}}}}} \right){\text{100 \% }}$ …… (2)

The mass of N is 28.02 g/mol.

The mass of ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is 96.0 g/mol.

Substitute these values in equation (2).

$\begin{aligned}{\text{\% composition of N}} &= \left( {\frac{{{\text{28}}{\text{.02 g/mol}}}}{{{\text{96}}{\text{.0 g/mol}}}}} \right){\text{100 \% }}\n&= {\text{29}}{\text{.1875 \% }} \n &\approx {\text{2}}{\text{.92 \%}}\n\end{aligned}$

Therefore the percentage composition by mass of nitrogen in ${\left( {{\text{N}}{{\text{H}}_{\text{4}}}} \right)_{\text{2}}}{\text{C}}{{\text{O}}_{\text{3}}}$ is 29.2 %.

Learn more:

Calculate the moles of chlorine in 8 moles of carbon tetrachloride: brainly.com/question/3064603
What is the concentration of alcohol in terms of molarity? brainly.com/question/9013318

Answer details:

Grade: Senior School

Chapter: Concentration terms

Subject: Chemistry

Keywords: (NH4)2CO3, N, nitrogen, mass, 2.92 %, 96.0 g/mol, 28.02 g/mol, nitrogen, hydrogen, carbon, oxygen, mass of N, mass of (NH4)2CO3.

The % composition of nitrogen is 29.166% ~ 29.2%. Thus option 2 is correct.

The percent composition of nitrogen in ammonium carbonate can be calculated as:

% Composition = $\rm (mass\;of\;element)/(mass\;of\lcompound)\;*\;100$