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3 years ago

If I have 0.725 moles of gas at a temperature of 105 K and a pressure of 3.75 atmospheres, what is the volume of the gas?

1 answer:

6 0

If I have 0.725 moles of gas at a temperature of 105 K and a pressure of 3.75 atmospheres the volume of the gas 1.66 litres.

Explanation:

Data given:

number of moles of the gas = 0.725

temperature = 105 K

pressure = 3.75 atm

volume of the gas =?

R = 0.08206 Latm/mole Kelvin

Applying the ideal gas law to calculate the volume of the given gas:

PV = nRT

rearranging the equation to calculate volume:

V = $\frac{nRT}{P}$

putting the values in the equation:

V = $\frac{0.08206 X 0.725 X 105}{3.75}$

V = 1.66 Litres.

At a temperature of 105 K and pressure of 3.75 atm, 0.725 moles of gas occupy 1.66 litres of volume.

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2) Give the number of lone pairs around the central atom and the molecular geometry of IF5. A) 0 lone pairs, square pyramidal D)

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Answer: D) 1 lone pair, square pyramidal

Explanation:

Formula used : $\text{Number of electrons}=\frac{1}{2}[V+N-C+A]$

where,

V = number of valence electrons present in central atom = 7

N = number of monovalent atoms bonded to central atom = 5

C = charge of cation = 0

A = charge of anion = 0

Now we have to determine the hybridization of the $IF_5$ molecule.

$\text{Number of electrons}=\frac{1}{2}\times [7+5+0-0]=6$

Bond pair electrons = 5

Lone pair electrons = 6-5 = 1

The number of electrons are 6 that means the hybridization will be $sp^3d^2$ and the electronic geometry of the molecule will be octahedral .

But as there are five atoms around the central iodine atom, the sixth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be square pyramidal.

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3 years ago

The ksp of pbi2 is 1.4 x 10-8. what is the molar solubility of lead(ii iodide in a solution of 0.400 m sodium iodide?

tino4ka555 [31]

The solubility product of a substance us calculated by the product of the concentration of the dissociated ions in the solution raise to the stoichiometric coefficient of the ions. Therefore, we need the dissociation reaction. For this, it will have the reaction:

PbI2 = Pb^2+ + 2I-

We solve as follows:

Ksp = [Pb2+][I-]^2 = 1.4 x 10-8
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The molar solubility would be 1.5x10^-3 M.

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3 years ago

The calorimeter pictured below shows the final temperature after calcium chloride was added to water. (The initial temperature w

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3 years ago

Read 2 more answers

A 0.590 gram sample of a metal, M, reacts completely with sulfuric acid according to:M(s) +H2SO4(aq) --> MSO4(aq) +H2(g)A vol

photoshop1234 [79]

Answer:

MM = 58.41 g

Explanation:

First, the data we have is according to the hydrogen which is exerting pressure. To solve this, we need to use the ideal gas equation:

PV = nRT (1)

the molar mass of any compound is calculated like this:

MM = m/n (2)

So, from (1) we solve for the moles (n) and then, this value is replace in (2).

However, before we do all that, we need to gather all the correct data.

All the species in the reaction are solid or aqueous state, with the exception of hydrogen, which is gaseous. Hydrogen is collected over water, therefore, is exerting some pressure too. The problem is not indicating if the acid or any other species is exerting pressure, so we will assume that only hydrogen and water are exerting pressure.

The total pressure exerted by the system would be:

P = Pw + PH2 (3)

We already know the total pressure which is 756 torr.

This experiment is taking place at 25 °C (298.15 K), and at this temperature, we have a reported value for water pressure which is 23.8 Torr.

Let's solve for PH2:

PH2 = P - Pw

PH2 = 756 - 23 = 733 Torr

Now, with this value, and the volume and temperature, we can calculate the moles of H2:

n = PV/RT

But first, let's convert the pressure to atm:

PH2 = 733 Torr / 760 torr * 1 atm = 0.9644 atm

now, solving for n:

n = 0.9644 * (0.255) / 0.082 * 298.15

n = 0.0101 moles

Now that we have the moles, we know that the metal and the hydrogen has a mole ratio of 1:1 according to the reaction, so, this means that:

moles M = moles H2 = 0.0101 moles

We have the moles of the metal and the mass, we can calculate the molar mass using expression (2):

MM = 0.590/0.0101

MM = 58.41 g/mol

This is the molar mass of the metal

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3 years ago