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Alenkasestr [34]
3 years ago
9

Argon has a pressure of 34.6 atm. It is transferred to a new tank with a volume of 456 L and pressure of 2.94 atm. What was the

volume of the original container?
Chemistry
1 answer:
NemiM [27]3 years ago
3 0

Answer:

38.75 L

Explanation:

From the question,

Applying Boyles Law,

PV = P'V'....................... Equation 1

Where P = Original pressure of the Argon gas, V = Original Volume of Argon gas, P' = Final pressure of Argon gas, V' =  Final Volume of Argon gas.

make V the subject of the equation

V = P'V'/P.................... Equation 2

Given: P = 34.6 atm, V' = 456 L, P' = 2.94 atm.

Substitute these values into equation 2

V = (456×2.94)/34.6

V = 38.75 L

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When dissolving a solid or liquid, as the temperature of the solvent increases, the rate of dissolution?
Alinara [238K]

Answer:A. Increases

Explanation:

Heating or an increase in temperature increases the kinetic energy of particles thereby increasing their motion and how they relate and react with one another.

Increase in the temperature of the solvent is directly proportional to the rate of dissolution. The rate of dissolution increases due to the increase in kinetic energy. This makes the solvent particles interact faster with the solute particles thereby increasing the dissolution rate.

7 0
3 years ago
Suppose we have a 12.2 L sample containing 0.50 mol oxygen gas at a pressure of 1 atm and a temperature of 25 degrees celcius. I
snow_lady [41]

Answer:

c. 8.1 L

Explanation:

Given that:-

Moles of oxygen gas = 0.50 mol

According to the reaction shown below as:-

3O_2\rightarrow 2O_3

3 moles of oxygen gas on reaction gives 2 moles of ozone

Also,

1 mole of oxygen gas on reaction gives 2/3 moles of ozone

So,

0.50 mole of oxygen gas on reaction gives \frac{2}{3}\times 0.50 moles of ozone

Moles of ozone = 0.3333 mol

Pressure = 1 atm

Temperature = 25.0 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (25.0 + 273.15) K = 298.15 K  

Volume = ?

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

1 atm × V = 0.3333 mol × 0.0821 L.atm/K.mol × 298.15 K  

⇒V = 8.1 L

6 0
2 years ago
2.93 mol of MgF2 to grams
mojhsa [17]

The mass of 1.72 mol of magnesium fluoride is 107 grams.

To determine the mass of 1.72 mol of magnesium fluoride, we first need the chemical formula of magnesium fluoride. Magnesium forms a +2 ion (Mg+2) and fluoride forms a -1 ion (F-1). Since all compounds formed from ions have to be electrically neutral, we need 2 fluoride ions and 1 magnesium ion. Therefore, the formula for magnesium fluoride is MgF2.

Now we need to determine the molar mass of the compound from the molar mass values from the periodic table. Let's use a table to calculate this molar mass.

Molar mass of MgF2

Element Molar Mass (g/mol) Quantity Total (g/mol)

Mg 24.31 1 24.31

F 19.00 2 38.00

Total molar mass of MgF2 = 24.31 g/mol + 38.00 g/mol = 62.31 g/mol

This is the mass of one mole of the substance. If we have 1.72 mols of it, we multiply 1.72 by 62.31.

1.72 mol (62.31 g/mol) = 107 grams

We rounded to 107 to keep the correct number of significant digits in our answer.

8 0
2 years ago
2. What is the mass of one mole of Na?
borishaifa [10]
Sodium, Atomic mass: 22.989769 g
You can see in a periodic table
5 0
3 years ago
Notice that "SO4" appears in two different places in this chemical equation. SO42− is a polyatomic ion called "sulfate." What nu
vichka [17]

Answer:

3.

Explanation:

Hello,

In this case, it is convenient to write the chemical reaction as:

CaSO_4+AlCl_3\rightarrow CaCl_2+Al_2(SO_4)_3

Which balanced turns out:

3CaSO_4+2AlCl_3\rightarrow 3CaCl_2+Al_2(SO_4)_3

Thus the number that should be in front of the calcium sulfate is 3 in order to balance the reaction.

Best regards.

8 0
2 years ago
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