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2 years ago

Which of the following is best described as an acid-base reaction?

Chemistry

1 answer:

seraphim [82]2 years ago

4 0

The reaction which represents an acid-base reaction is: HNO3(aq) + NH3(aq) → NH4*(aq) + NO3(aq).

<h3>What is an acid-base reaction?</h3>

An acid-base reaction is a reaction in which a substance donate protons to another substance which then accepts the proton.

An acid-base reaction usually involves the formation of a salt.

From the given reactions, the acid-base reaction is given below:

HNO3(aq) + NH3(aq) → NH4*(aq) + NO3(aq)

In the given reaction, HNO3 donates a proton and NH3 accepts the proton.

Therefore, the reaction which represents an acid-base reaction is: HNO3(aq) + NH3(aq) → NH4*(aq) + NO3(aq).

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Balance the redox reaction in alkaline medium & identify the oxidizing & reducing agents

Darya [45]

The balanced redox equation of the reaction is given below:

I⁻ + 2 MnO₄ + H₂O → IO₃⁻ + 2 MnO₂ + 2 OH⁻

The oxidizing agent is MnO₄ while the reducing agent is I⁻.

<h3>What are redox equations?</h3>

Redox equations are equations in which oxidation and reduction reactions occur together.

Redox reactions can take place in alkaline or acidic mediums.

The balanced redox equation of the reaction is given below:

I⁻ + 2 MnO₄ + H₂O → IO₃⁻ + 2 MnO₂ + 2 OH⁻

The oxidizing agent is MnO₄ while the reducing agent is I⁻

In conclusion, a balanced redox equation is one in which the atoms and the change in oxidation state is equal on both sides of the reaction.

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8 0

2 years ago

What is the density of 2.5 g of gaseous sulfur held at 130. kPa and 10.0 degrees Celsius?

worty [1.4K]

Use ideal gas equation: pV = nRT

Now pass n to mass: n = mass / MM .... [MM is the molar mass]

pV = [mass/MM]*RT =>mass/V = [p*MM] / RT and mass / V = density

p= 130 kPa = 130,000 Pa = 130,00 joule / m^3
T = 10.0 ° + 273.15 = 283.15 k
MM of sulfur (S) = 32 g/mol = 32000 kg/mol

density = 130,000 Pa * 32000kg/mol / [8.31 joule / mol*k * 283.15 k] = 1.77*10^6 kg/m^3 = 1.77 g/L ≈ 1.8 g/L

Then, I do not get any of the option choices.

Is it possbile that the pressure is 13.0 kPa instead 130. kPa? If so the answer would be 18 g/L

Note that the mass is not used. You do not need it unless you are asked for the volume, which is not the case.

4 0

4 years ago

Read 2 more answers

Calculate the mass of 45.0 L of Cl₂ at

amid [387]

The mass of 45.0 L of Cl₂ at 87.0° C and 950 mm Hg is 134.7214 g.

Volume = 45.0 L

Temperature = = (87.0 + 273) K = 360 K

Pressure = 950 mm Hg (1 mm Hg = 0.00131579 atm) = 1.25 atm

The formula used to calculate moles is as follows.

∴PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into the above formula as follows:

∴ PV = nRT

=> 1.25 atm × 45.0 L = n × 0.0821 L atm/mol K × 360K

=> n = 1.25 atm × 45.0 L / n × 0.0821 L atm/mol K × 360K

=> n = 56.25 / 29.556 mol

=> n = 1.90 mol

Moles is the mass of a substance divided by its molar mass. So, the mass of Cl₂ (molar mass = 70.906 g/mol) is calculated as follows:

∴ Moles = mass / molar mass

=> 1.90 mol = mass / 70.906 g/mol

=> mass = 134.7214 g

Thus, we can conclude that the mass of 45.0 L of Cl₂ at 87.0° C and 950 mm Hg is 134.7214 g.

To know more about the Ideal Gas Law :

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5 0

1 year ago

Read 2 more answers

30. The density of an unknown gas at 27°C and 2 atm pressure is equal with density of N2 gas at

Zanzabum

Answer:

Molar mass of the unknown gas is 64.6 g/mol

Explanation:

Let's think this excersise with the Ideal Gases Law.

We start from the N₂. At STP conditions we know that 1 mol of anything occupies 22.4L.

We apply: P . V = n . R . T

5 atm . V = 1 mol . 0.082 . 325K

V = (1 mol . 0.082 . 325K) / 5 atm = 5.33 L

It is reasonable to say that, if we have more pressure, we may have less volume.

As this is the volume for 1 mol of N₂, our mass is 28 g. Then, the density of the nitrogen and the unknown gas is 28 g/5.33L = 5.25 g/L

Our unknown gas has, this density at 27°C and 2 atm.

If we star from this, again: 1 mol of any gas occupy 22.4L at STP, we can calculate the volume for 1 mol at those conditions:

P₁ . V₁ / T₁ = P₂ . V₂ / T₂

1 atm . 22,4L / 273K = 2 atm . V₂ / 300K

Remember that the value for T° is Absolute (T°C + 273)

[ (1 atm . 22.4L / 273K) . 300K] / 2 atm = V₂ → 12.3L

This is the volume for 1 mol of the unknown gas at 2 atm and 27°C

We use density to determine the mass: 12.3 L . 5.25 g/L = 64.6 g

That's the molar mass: 64.6 g/mol

6 0

3 years ago

What are the conditions that are required for electrical energy to be present in an electrical circuit?

Nat2105 [25]

Answer:

a supply of electric charges which are free to flow, some form of push to move the charges through the circuit and a pathway to carry the charges.

Explanation:

There's your answer have a good day

6 0

2 years ago