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Neko [114]
3 years ago
6

To what temperature does a 250 ml cylinder containing 0.40 grams of helium gas need to be collected in order for the pressure to

be 253.25 kPa?
Please show work.
Chemistry
1 answer:
VMariaS [17]3 years ago
6 0

Answer:

T =76.13 K

Explanation:

Given data:

Temperature of gas = ?

Volume of gas = 250 mL(250/1000 = 0.25 L)

Mass of helium = 0.40 g

Pressure of gas = 253.25 kpa (253.25/101 = 2.5 atm)

Solution:

Formula:

PV = nRT

First of all we will determine the number of moles of helium.

Number of moles = mass/ molar mass

Number of moles = 0.40 g/ 4 g/mol

Number of moles = 0.1 mol

Now we will put the values.

R = general gas constant = 0.0821 atm.L/ mol.K

T = PV/nR

T =2.5 atm× 0.25 L /0.1 mol ×0.0821 atm.L/ mol.K

T = 0.625  /0.00821/K

T =76.13 K

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denpristay [2]

Answer:

PROTON AND NEUTRON

Explanation:

  • The mass of proton is : 1.67*10^{-27}kg

A proton is one of the main particles that make up the atom . The other two particles are neutron and electron. Protons are found in the nucleus of the atom.This is a tiny , dense region at the centre of the atom. Protons have a positive charge of one (+1) and a mass of 1 atomic mass unit ( amu ) , which is about 1.67*10^{-27}kg. Together with neutrons , they make up virtually all of the mass of an atom.

  • The  mass of neutron is also approximately: 1.67*10^{-27}kg but a little more than that .

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6 0
3 years ago
The equilibrium constant for the gas-phase isomerization of borneol (c10h17oh) to isoborneol at 503 k is 0.106. a mixture consis
Dimas [21]
The solution is as follows:

K = [Partial pressure of isoborneol]/[Partial pressure of borneol] = 0.106

The molar mass of isoborneol/borneol is 154.25 g/mol

Mol isoborneol = 15 g/154.25 = 0.0972 mol
Mol borneol = 7.5 g/154.25 = 0.0486 mol

Use the ICE approach

        borneol  →  isoborneol
I         0.0972           0.0486
C         -x                     +x
E     0.0972 - x        0.0486 + x

Total moles = 0.1458

Using Raoult's Law,
Partial Pressure = Mole fraction*Total Pressure
[Partial pressure of isoborneol] = [(0.0972-x)/0.1458]*P
[Partial pressure of borneol] = [(0.0486+x/0.1458)]*P

0.106 = [(0.0972-x)/0.1458]*P/ [(0.0486+x/0.1458)]*P
Solving for x,
x = 0.0832 

Thus,
<em>Mol fraction of borneol = (0.0486+0.0832)/0.1458 = 0.904</em>
<em>Mol fraction of isoborneol = (0.0972-0.0832)/0.1458 = 0.096</em>
6 0
3 years ago
Identify the Lewis acid in the following reaction: Cr3+(aq)+6H2O(aq)⇌Cr(H2O)63+(aq)
Nostrana [21]
In the reaction,
Cr3+(aq) + 6H2O -------> [Cr(H2O)6]3+(aq)
Cr3+ IS THE LEWIS ACID H2O is the Lewis base.
A Lewis acid is a compound or chemical that accepts a lone pair of electrons. In the above equation, Cr3+ is accepting the lone pair of electrons.
3 0
3 years ago
Read 2 more answers
An expandable container of oxygen has a volume of 30.0mL at a pressure of 36.7psi. If the pressure of the oxygen is reduced to 2
ELEN [110]

Answer:44.04mL

Explanation:Parameters given

V1 = 30.0mL

P1 = 36.7psi

P2 = 25.0psi

V2 = ??

From Boyle's gas law, which states that "the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature"

This means that,

the pressure of a gas tends to increase as the volume of the container decreases, and also the pressure of a gas tends to decrease as the volume of the container increases.

Mathematically, Boyle's can be represented as shown below

P= k/V

Where P = Pressure, V = Volume and k is constant

Therefore,

PV = k

P1V1 = P2V2 =PnVn

Using the formula

P1V1 = P2V2

V2 = P1V1/P2

V2 = (36.7psi × 30.0mL) / 25.0psi

V2 = 1101.0/25.0

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3 years ago
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Please help!!! Stoich Question
Greeley [361]

Answer:

4KO₂ + 2CO₂ -> 2K₂CO₃ + 3O₂

<u> Step 1: Find the moles of O₂.</u>

n(O₂) = mass/ Mr.

n(O₂) = 100 / 32 = 3.125 mol

<u>Step 2: Find the ratio between KO₂ and O₂.</u>

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          4        :       3

        4/3       :       1

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Thus now we know, to produce 100 g of O₂, we need 4.167mol of KO₂

<u>Step 3: Find the mass of KO₂:</u>

<u />

mass = mol * Mr. (KO₂)

Mass = 4.167* 71.1

Mass = 296.25 g

5 0
2 years ago
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