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4 years ago

What is the pressure of 5.0 mol nitrogen gas in a 2.0 L container at 286 K

1 answer:

5 0

The "Ideal Gas Law Equations" is
$PV=nRT$
P= Pressure (in Pascals)
V=Volume (in Liters)
n=amount, or number (in moles)
R= 8.3145 $\frac{Pascals*Liters}{Moles*Kelvin}$ or $\frac{PaL}{molK}$
T= Temperature (In Kelvin)

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

Plug into the equation and you're good!
$P=\frac{nRT}{V}$
$P =\frac{(5mol)(8.3145)(286K)}{2L}$
$P=5944.8675Pa$

If your teacher cares about sig figs,
2 sig figs (significant figures)
$P=5900Pa$

For other units of pressure,
1 atm = 760 mmHG = 760 Torr = 101326 Pa = 1.01325 bar

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How many grams C3H7OH can be made by reacting with 7.3L of CO2 at STP

Komok [63]

Answer:

6.54g of C3H7OH

Explanation:

Step 1:

Determination of the number of mole of CO2 that occupy 7.3L at stp.

This can be obtained as follow:

1 mole of a gas occupy 22.4L at stp.

Therefore, Xmol of CO2 will occupy 7.3L at stp i.e

Xmol of CO2 = 7.3/22.4

Xmol of CO2 = 0.326 mole.

Therefore, 0.326 mole of CO2 was used in the reaction.

Step 2:

The balanced equation for the reaction. This is given below:

6CO2 + 8H2O —> 2C3H7OH + 9O2

Step 3:

Determination of the number of mole of C3H7OH produced from the reaction. This is illustrated below:

From the balanced equation above,

6 moles of CO2 reacted to produce 2 moles of C3H7OH.

Therefore, 0.326 mole of CO2 will react to produce = (0.326 x 2)/6 = 0.109 mole of C3H7OH.

Step 4:

Conversion of 0.109 mole of C3H7OH to grams. This is illustrated below:

Number of mole of C3H7OH = 0.109 mole.

Molar mass of C3H7OH = (12x3)+ (7x1) + 16 + 1 = 60g/mol

Mass of C3H7OH =..?

Mass = mole x molar mass

Mass of C3H7OH = 0.109 x 60

Mass of C3H7OH = 6.54g.

Therefore, 6.54g of C3H7OH is produced from the reaction.

5 0

3 years ago

What is an asteroid?

LUCKY_DIMON [66]

Asteroids are rocky space debris that are formed from interspacial collisions and collection of dusty particles. our solar system has an enormous asteroid belt between Mars and Jupiter.

Jupiter also has more local asteroids that are locked to its gravitational pull.

Not to be confused with a comet or meteor.

5 0

3 years ago

Read 2 more answers

How many moles of O2 are needed to produce 3.95 moles of Fe2O3

Minchanka [31]

Answer:

4Fe+3O2- 2Fe2O3

the ratio: 3:2

x:3.95

x=5.92 moles of O2

5 0

2 years ago

A mixture of h2 and n2 has a density of 0.216 at 300k and 500 torr. what is the mole fraction composition of the mixture

natta225 [31]

We know that:
number of moles (n) = mass / molar mass

Now, from the general law of gases:
PV = nRT
where:
P is the pressure = 500 torr = 0.65 atm
V is the volume
n is the number of moles
R is the gas constant = 0.082
T is the temperature = 300 k
We will just rearrange this equation as follows:
P = nRT / V
Then we will substitute n with its equivalent equation mentioned at the beginning:
P = (mass x R x T) / (volume x molar mass) ......> equation I
Now, we know that:
density = mass / volume
We will substitute (mass/volume) in equation I with density as follows:
P = (density x R x T) / molar mass
Rearrange this equation to get the mass as follows:
molar mass = dRT/P = (0.216 x 0.082 x 300) / 0.65 = 8.4738 grams

From the periodic table:
molecular mass of hydrogen = 1 grams
molecular mass of nitrogen = 14 grams
Therefore:
molar mass of hydrogen = 2 x 1 = 2 grams
molar mass of nitrogen = 2 x 14 = 28 grams

We can assume that the number of moles of of each element is y.
We can thus build up the following equation:
2y + 28y = 8.4738
30y = 8.4738
y = 0.28246

Therefore:
mole fraction of hydrogen = 2 x 0.28246 = 0.56492
mole fraction of nitrogen = 28 x 0.28246 = 7.90888

4 0

4 years ago

Which of the following cannotbe considered a single phase? a heterogeneous mixture a pure solid a homogeneous mixture a pure liq

MrRa [10]

A heterogeneous mixture cannot be considered a single phase

4 0

3 years ago