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3 years ago

A neighbor wants to use his backyard garden to

Chemistry

1 answer:

Anastaziya [24]3 years ago

4 0

Answer:

No, it is not

Explanation:

The reason for this answer is below

To conduct an experiment/investigation that involves the use of specific amounts of carbon dioxide and water by plants, one needs a controlled environment where the amount of carbon dioxide and water made available to the plant can be monitored and regulated as desired by the experimental design. The neighbor's backyard cannot provide this controlled environment and thus it is a bad idea.

Note that the neighbor's backyard cannot provide the controlled environment because the amount of carbon dioxide the plants will be exposed to there cannot be regulated as this is the carbon dioxide from the atmosphere and also the plants could get additional water from midnight dew which cannot be regulated also.

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True or False: It is OK to use wet glassware for the aspirin synthesis without potentially affecting your yield

vesna_86 [32]

Answer:

False

Explanation:

Laboratory synthesis of aspirin is done by the acetylation of salicylic acid with the help of acetic anhydride .

As , the acid anhydride is very sensitive to moisture , as it can hydrolyze into two molecules of acids,

Hence , the reaction involving acid anhydride are conducted in anhydrous solvents .

Hence ,

if water is present in the glassware then , some of the acetic anhydride is wasted , Which in turns reduces the yield than that expected .

5 0

3 years ago

Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq)

Svetach [21]

Answer:

The solution 0.010 M has a higher percent ionization of the acid.

Explanation:

The percent ionization can be found using the following equation:

$\% I = \frac{[H_{3}O^{+}]}{[CH_{3}COOH]} \times 100$

Since we know the acid concentration in the two cases, we need to find [H₃O⁺].

By using the dissociation of acetic acid in the water we can calculate the concentration of H₃O⁺ in the two cases:

1. Case 1 (0.1 M):

CH₃COOH(aq) + H₂O(l) ⇄ CH₃COO⁻(aq) + H₃O⁺(aq) (1)

0.1 - x x x

$Ka = \frac{[CH_{3}COO^{-}][H_{3}O^{+}]}{[CH_{3}COOH]}$ (2)

Where:

Ka: is the dissociation constant of acetic acid = 1.7x10⁻⁵.

$1.7 \cdot 10^{-5} = \frac{x^{2}}{0.1 - x}$

$1.7 \cdot 10^{-5}*(0.1 - x) - x^{2} = 0$

By solving the above equation for x we have:

x = 1.29x10⁻³ M = [CH₃COO⁻] = [H₃O⁺]

Hence, the percent ionization is:

$\% I = \frac{1.29 \cdot 10^{-3} M}{0.1 M} \times 100 = 1.29 \%$

2. Case 2 (0.01 M):

The dissociation constant from reaction (1) is:

$Ka = \frac{[CH_{3}COO^{-}][H_{3}O^{+}]}{[CH_{3}COOH]}$

With [CH₃COOH] = 0.01 M

$1.7 \cdot 10^{-5} = \frac{x^{2}}{0.01 - x}$

$1.7 \cdot 10^{-5}*(0.01 - x) - x^{2} = 0$

By solving the above equation for x:

x = 4.04x10⁻⁴ M = [CH₃COO⁻] = [H₃O⁺]

Then, the percent ionization for this case is:

$\% I = \frac{4.04 \cdot 10^{-4} M}{0.01 M} \times 100 = 4.04 \%$

As we can see, the solution 0.010 M has a higher percent ionization of the acetic acid.

Therefore, the solution 0.010 M has a higher percent ionization of the acid.

I hope it helps you!

4 0

3 years ago

If a sample of Fe2O3, (rust) contains 30.00g of iron, how many grams of oxygen should it have?

bixtya [17]

Where are the answer choices

7 0

3 years ago

Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) Which ion would NOT be present in

Allisa [31]

Answer:

The question is incomplete and confusing.

In the complete ionic equation you write all the ions that are formed. Those are: Pb²⁺, NO₃⁻, K⁺, and I⁻. They all are present in the complete ionic equation.

In the net ionic equation, the spectator ions do not appear. They are: NO₃⁻ and K⁺. They would not be present in the net ionic equation, but they do in the complete ionic equation.

See below the details.

Explanation:

Which compound will not form ions?

1. Write the balanced molecular equation:

Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO₃(aq)

2. Write the ionizations for the ionic aqueous compounds:

Pb(NO₃)₂(aq) → Pb⁺²(aq) + 2NO₃⁻(aq)

2KI(aq) → 2K⁺(aq) + 2I⁻(aq)

2KNO₃(aq) → 2K⁺(aq) + 2NO₃⁻(aq)

3. Write the complete ionic equation:

Pb⁺²(aq) + 2NO₃⁻(aq) + 2K⁺(aq) + 2I⁻(aq) → PbI₂(s) + 2K⁺(aq) + 2NO₃⁻(aq)

Hence, since PbI₂(s) does not ionize, but stays in solid form, it will not form ions.

All, Pb⁺², NO₃⁻, K⁺, and I⁻ will be present in the total ionic equation.

It is in the net ionic equation that the spectator ions are removed. Those, are NO₃⁻ and K⁺, because they are on both sides of the complete ionic equation.

3 0

3 years ago

Why does thermal energy decreases when potassium is dissolved in water

Levart [38]

Answer:

The process of dissolving can be endothermic (temperature goes down) or exothermic (temperature goes up).

When water dissolves a substance, the water molecules attract and “bond” to the particles (molecules or ions) of the substance causing the particles to separate from each other.

The “bond” that a water molecule makes is not a covalent or ionic bond. It is a strong attraction caused by water’s polarity.

It takes energy to break the bonds between the molecules or ions of the solute.

Energy is released when water molecules bond to the solute molecules or ions.

If it takes more energy to separate the particles of the solute than is released when the water molecules bond to the particles, then the temperature goes down (endothermic).

If it takes less energy to separate the particles of the solute than is released when the water molecules bond to the particles, then the temperature goes up (exothermic).

Explanation:

8 0

3 years ago