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3 years ago

The Molar mass(M.w) in g/mol of 6.3 grams of an ideal gas that placed in 5.0 L tank at ST

Chemistry

1 answer:

BigorU [14]3 years ago

7 0

Answer:

28 g/mol, N2

Explanation:

Given data:

Volume of gas = 5.0 L

Mass of gas = 6.3 g

Pressure = 1 atm

Temperature = 273 K

Molar mass of gas = ?

Solution:

We will calculate the density first.

d = mass/ volume

d = 6.3 g/ 5.0 L

d = 1.26 g/L

Molar mass:

d = PM/RT

M = dRT/P

M = 1.26 g/L× 0.0821 atm.L/mol.K × 273 K/ 1 atm

M = 28 g/mol

Molar mass of N₂ is 28 g/mol thus given gas is N₂.

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A 6.00 L vessel contains 20.0 g of PCl3 and 3.15 g of O2 at 15.0 ∘C. The vessel is heated to 210 ∘C, and the contents react to g

dusya [7]

Answer: The final pressure in the vessel will be 0.965 atm

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For phosphorus trichloride:

Given mass of phosphorus trichloride = 20.0 g

Molar mass of phosphorus trichloride = 137.3 g/mol

Putting values in equation 1, we get:

$\text{Moles of phosphorus trichloride}=\frac{20.0g}{137.3g/mol}=0.146mol$

For oxygen gas:

Given mass of oxygen gas = 3.15 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of oxygen gas}=\frac{3.15g}{32g/mol}=0.098mol$

The chemical equation for the reaction of phosphorus trichloride and oxygen gas follows:

$2PCl_3+O_2\rightarrow 2POCl_3$

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride reacts with 1 mole of oxygen gas

So, 0.146 moles of phosphorus trichloride will react with = $\frac{1}{2}\times 0.146=0.073mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, phosphorus trichloride is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride produces 2 moles of $POCl_3$

So, 0.146 moles of phosphorus trichloride will produce = $\frac{2}{2}\times 0.146=0.146mol$ of $POCl_3$

To calculate the pressure of the vessel, we use the equation given by ideal gas follows:

$PV=nRT$

where,

P = pressure of the vessel = ?

V = Volume of the vessel = 6.00 L

T = Temperature of the vessel = $210^oC=[210+273]K=483K$

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

n = number of moles = 0.146 moles

Putting values in above equation, we get:

$P\times 6.00L=0.146mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 483K\\\\P=\frac{0.146\times 0.0821\times 483}{6.00}=0.965atm$

Hence, the final pressure in the vessel will be 0.965 atm

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4 years ago

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What will the presence of H+ ions in a solution cause?

vodka [1.7K]

The H+ will react with Magnesium to release hydrogen Gas under the equation Mg + 2H+ --> Mg(2+) + H2(g)

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3 years ago

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Why does a biker have to peddle harder to travel at a constant speed into the

Anna35 [415]

Answer:

wind has resistance, 10 mph of wind has more than 0 mph

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3 years ago

Which of these might affect whether or not a particular chemical reaction occurs?

Vinvika [58]

Your answer would be D.

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3 years ago

A gas occupies 5.31 liters at a pressure of 0.55 atm. Determine the volume at standard pressure.

yuradex [85]

Answer:

Option A; V = 2.92 L

Explanation:

If we assume a lot of things, like:

The gas is an ideal gas.

The temperature is constant.

The gas does not interchange mass with the environment.

Then we have the relation:

P*V = n*R*T = constant.

Where:

P = pressure

V = volume

n = number of moles

R = constant of the ideal gas

T = temperature.

We know that when P = 0.55 atm, the volume is 5.31 L

Then:

(0.55 atm)*(5.31 L) = constant

Now, when the gas is at standard pressure ( P = 1 atm)

We still have the relation:

P*V = constant = (0.55 atm)*(5.31 L)

(1 atm)*V = (0.55 atm)*(5.31 L)

Now we only need to solve this for V.

V = (0.55 atm/ 1 atm)*(5.31 L) = 2.92 L

V = 2.92 L

Then the correct option is A.

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3 years ago