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2 years ago

How many moles of a gas are contained in 2.085 L at STP?

1 answer:

muminat2 years ago

4 0

Answer /-

A.0.0931 mol

from ideal gas equation ,

We have ,

PV = nRT

Where P stands where pressure of gas.
We know that pressure of gas at STP = 1 atm

V stands for volume of gas , given Volume is 2.085 L

R stands for gas constant , R = 0.0821

And T stands for absolute temperature and measured in kelvin,T=273K

Now ,

PV = nRT

n = PV/RT

Refer attachment for working

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A gas has density 2.41 g/liter at 25°C and 770 mm Hg. Calculate it's molecular mass (R = 0.0821 L atm.mol-1K-1

Evgesh-ka [11]

Answer:

Explanation:

Given : Density - 2.41 g/liter

Temperature - 25° C

Pressure : 770 mm Hg

R = 0.0821 L atm mol-¹K-¹

Find : Molecular mass of gas

Solution : Ideal gas equation with respect to density will be : PM = dRT. In the formula, P is pressure, M is molecular mass, d is density, R is gas constant and T is temperature.

Keeping the values in equation-

Pressure : 770 mm Hg = 1 atm

Temperature : 273 + 25 = 298 K

M = dRT/P

M = (2.41*0.0821*298)/1

M = 58.96 gram/mol

Thus, the molecular mass of gas is 58.96 gram/mol.

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3 years ago

A mixture of reactants and products for the reaction shown below is at

zavuch27 [327]

If the volume of the container were increased to 4.0 L, more N₂ and H₂ would be produced (Option D)

<h3>What is chemical equilibrium? </h3>

This is simply defined as a state in a chemical system where there is no observable change in the properties of the system with time.

<h3>Principle of chemical equilibrium </h3>

A French scientist postulated a principle which helps us to understand a chemical system in equilibrium.

The principle states as follow:

If a an external constraint such as change in temperature, pressure or concentration is imposed on a system in equilibrium, the equilibrium will shift so as to neutralize the effect.

<h3>How to determine what will happen if the volume of the container is increased from 2 L to 4 L</h3>

From the principle given above, we can see that volume does not affect equilirium position.

However, from Boyle's law, we understood that pressure and volume are in invest relationship.

Thus, increasing volume simply means decreasing pressure.

A decrease in pressure will favors the side where there is an increase in volume.

Let us consider the equation from the question:

N₂(g) + 3H₂(g) <=> 2NH₃(g)

Volume of reactants = 1 + 3 = 4 L
Volume of products = 2 L

Thus, we can conclude that increasing the volume (i.e decreasing the pressure) of the reaction will favors the backward reaction, hence, more N₂ and H₂ would be produced.

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2 years ago

How many moles of Cl- ions are needed to completely combine with 0.25 moles of Mg+2 ions?

Mnenie [13.5K]

<span>The number of moles of Cl- ions needed to combine completely with 0.25 mole of Mg+2 ions is:
0.50.</span>

4 0

3 years ago

In which state of matter does heat travel fastest and slowest?

MariettaO [177]

Answer:

Heat travels faster in solids.

Heat travels slower in gases.

Explanation:

5 0

3 years ago

I NEED HELP ASAP! PLEASE BE GENUINE

love history [14]

1. The molar mass of the unknown gas obtained is 0.096 g/mol

2. The pressure of the oxygen gas in the tank is 1.524 atm

<h3>Graham's law of diffusion </h3>

This states that the rate of diffusion of a gas is inversely proportional to the square root of the molar mass i.e

R ∝ 1/ √M

R₁/R₂ = √(M₂/M₁)

<h3>1. How to determine the molar mass of the gas </h3>

Rate of unknown gas (R₁) = 11.1 mins
Rate of H₂ (R₂) = 2.42 mins
Molar mass of H₂ (M₂) = 2.02 g/mol

Molar mass of unknown gas (M₁) =?

R₁/R₂ = √(M₂/M₁)

11.1 / 2.42 = √(2.02 / M₁)

Square both side

(11.1 / 2.42)² = 2.02 / M₁

Cross multiply

(11.1 / 2.42)² × M₁ = 2.02

Divide both side by (11.1 / 2.42)²

M₁ = 2.02 / (11.1 / 2.42)²

M₁ = 0.096 g/mol

<h3>2. How to determine the pressure of O₂</h3>

From the question given above, the following data were obtained:

Volume (V) = 438 L
Mass of O₂ = 0.885 kg = 885 g
Molar mass of O₂ = 32 g/mol
Mole of of O₂ (n) = 885 / 32 = 27.65625 moles
Temperature (T) = 21 °C = 21 + 273 = 294 K
Gas constant (R) = 0.0821 atm.L/Kmol

Pressure (P) =?

The pressure of the gas can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

Divide both side by V

P = nRT / V

P = (27.65625 × 0.0821 × 294) / 438

P = 1.524 atm

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2 years ago