Chemistry College

if the waste you have contains 100.0 grams of silver nitrate, how many mols of silver nitrate is this

Answers

Answer 1
Final answer:

To find the number of moles of silver nitrate, divide the mass by the molar mass.

Explanation:

To determine the number of moles of silver nitrate in a given mass, we need to use the molar mass of silver nitrate. The molar mass of silver nitrate (AgNO3) is 169.88 g/mol.

Given that the waste contains 100.0 grams of silver nitrate, we divide the mass by the molar mass to find the number of moles:

Number of moles = Mass (g) / Molar mass (g/mol)

Number of moles = 100.0 g / 169.88 g/mol = 0.589 mol

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Answer 2

1. Given 100.0 grams of silver nitrate, we calculate it to be approximately 0.588 moles of silver nitrate.

2. According to the balanced chemical equation with copper, 0.294 moles of copper are needed to completely react with the silver nitrate. This ensures the reaction proceeds to completion.

To determine the number of moles of silver nitrate (AgNO₃) from the given mass, we use its molar mass:

Determine the molar mass of AgNO₃: 169.88 g/mol.Calculate the moles of silver nitrate:
Moles of AgNO₃ = mass / molar mass = 100.0 g / 169.88 g/mol ≈ 0.588 mol.

Next, we need to determine how many moles of copper (Cu) are needed to react completely with the silver nitrate.

The balanced chemical reaction between these two substances is:

2AgNO₃(aq) + Cu(s) → Cu(NO₃)₂ (aq) + 2Ag(s)

From the balanced equation, we see that 1 mole of Cu reacts with 2 moles of AgNO₃. Therefore, we use the stoichiometric ratio to find the required moles of copper:

Moles of Cu = 0.588 mol AgNO₃ * (1 mole Cu / 2 moles AgNO3) = 0.294 mol Cu

Correct question is: Answer the following :

1. If the waste you have contains 100.0 grams of silver nitrate, how many moles of silver nitrate is this? (Use the molar mass of the silver nitrate from above)
2. If you found that the waste contains 100.0 grams of silver nitrate, how many moles of copper would you need to completely react with all of the silver nitrate?

Related Questions

A certain shade of blue has a frequency of 7.03 × 1014 Hz. What is the energy of exactly one photon of this light?

Answers

4.66 x 10^-19 Joules The energy of a photon is E=hf Where E = Energy h = Planck's constant (6.62607004Ă—10â’34 J s) f = frequency of photon. So plug in the known values E = 6.62607004Ă—10â’34 J s * 7.03 x 10^14 1/s E = 4.65812724x10^-19 J Since we only have 3 significant figures, the rounded result is E = 4.66x10^-19 J

The energy of one photon of light with a frequency of 7.03 × 1014 Hz is approximately 4.65618 × 10-19 Joules. This is obtained using Planck's equation, E = hf, where E is the energy, h is Planck's constant and f is the frequency of the light.

Explanation:

The subject of this question is Physics. The student wants to know the energy of exactly one photon of light that has a frequency of 7.03 × 1014 Hz. We can use Planck's equation which relates the energy of photon, its frequency and Planck's constant (h = 6.626 × 10-34 J.s).

So, the energy (E) of the photon is given by the formula E = hf. Substituting the frequency (f = 7.03 × 1014 Hz) and Planck's constant into the formula gives E = (6.626 × 10-34 J.s)(7.03 × 1014 Hz) which gives approximately 4.65618 × 10-19 Joules. This is the energy of one photon of light with a frequency of 7.03 × 1014 Hz.

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