Can anyone explain how to do this?

Determine the pressure in atm exerted by 1 mole of methane placed into a bulb with a volume of 244.6 mL at 25°C. Carry out two c

Nuetrik [128]

The pressure in atm exerted by 1 mole of methane placed into a bulb with a volume of 244.6 mL at 25°C is 101.94atm.

<h3>How to calculate pressure?</h3>

The pressure of an ideal gas can be calculated using the following formula:

PV = nRT

Where;

P = pressure
V = volume
n = number of moles
R = gas law constant
T = temperature

According to information in this question;

T = 25°C = 25 + 273 = 298K
V = 244.6mL = 0.24L
R = 0.0821 Latm/Kmol

P × 0.24 = 1 × 0.0821 × 298

0.24P = 24.47

P = 24.47/0.24

P = 101.94atm

Therefore, the pressure in atm exerted by 1 mole of methane placed into a bulb with a volume of 244.6 mL at 25°C is 101.94atm.

Learn more about pressure at: brainly.com/question/11464844

3 0

3 years ago

Muriatic acid, HCl, is often used to remove rust. A solution of muriatic acid, HCl, reacts with Fe2O3 deposits on industrial equ

Alina [70]

Answer:

3L

Explanation:

Step 1:

The balanced equation for the reaction.

Fe2O3(s) + 6HCl(aq) → 2FeCl3(aq) + 3H2O

Step 2 :

Determination of the masses of HCl and Fe2O3 that reacted from the balanced equation. This is illustrated below:

Molar mass of Fe2O3 = 159.70g/mol

Molar mass of HCl = 36.46 g/mol

Mass of HCl from the balanced equation = 6 x 36.46 = 218.76g

From the balanced equation above,

159.70g of Fe2O3 reacted with 218.76g of HCl

Step 3:

Determination of the mass of HCl needed to react with 439g of Fe2O3. This is illustrated below:

From the balanced equation above,

159.70g of Fe2O3 reacted with 218.76g of HCl.

Therefore, 439g of Fe2O3 will react with = (439 x 218.76) /159.70 = 601.35g of HCl.

Step 4:

Conversion of 601.35g of HCl to mole. This is illustrated below:

Molar mass of HCl = 36.46 g/mol

Mass of HCl = 601.35g

Number of mole = Mass/Molar Mass

Number of mole of HCl = 601.35/36.46

Number of mole of HCl = 16.49 moles

Step 5:

Determination of the volume of the HCl that reacted.

This is illustrated below:

Mole of HCl = 16.49 moles

Molarity of HCl = 5.50 M

Volume =?

Molarity = mole /Volume

Volume = mole /Molarity

Volume = 16.49/5.5

Volume of HCl = 3L

Therefore the volume of HCl needed for the reaction is 3L

5 0

3 years ago

Cuántos moles hay en 17.5 gramod de ZnCl2

Aliun [14]

Explanation:

Zn=65

Cl2= 35+35=70

65+70=135g

1 mole ZnCl2 = 135g

x mole = 17.5g

17.5g × 1 mole/ 135g= 0.129 moles en 17.5g de ZnCl2

4 0

3 years ago

How many grams Glycylglycine (molecular mass 132.119 grams/mole) are required to make 1 liter at 0.5 Molar concentration. If you

SOVA2 [1]

Explanation:

The given data is as follows.

Concentration of solution = 0.5 M

Volume of solution = 1 L

Molar mass of Glycylglycine = 132.119 g/mol

As molarity is the number of moles present in liter of solvent.

Mathematically, Molarity = $\frac{\text{No. of moles}}{\text{Volume}}$

Hence, calculate the number of moles as follows.

No. of moles = Molarity × Volume

= $0.5 M \times 1 L$

= 0.5 mol

Therefore, mass of glycylglycine = mol × molar mass

= $0.5 mol \times 132.119 g/mol$

= 66.06 g

Thus, we can conclude that 66.06 g glycylglycine is required.

8 0

3 years ago

Inelastic collisions occur in a. Real and ideal gases

IceJOKER [234]

<span>c. Real gases and fusion reactions </span>

8 0

3 years ago