The pressure the gas exert the walls of the container will decrease because the gas particles hit the wall of the container

1 answer:

5 0

The statement is false. The pressure of a gas do not decrease as the gas molecules hit the walls of the container. According to the Kinetic Molecular Theory, collisions of the gas molecules or with the walls of the container are perfectly elastic. This means that energy is not lost as the molecules collide with each other or with the walls of the container.

You might be interested in

When aqueous solutions of potassium fluoride and hydrochloric acid are mixed, an aqueous solution of potassium chloride and hydr

Semmy [17]

Answer:

K⁺ (aq) + F⁻ (aq) + H⁺ (aq) + Cl⁻ (aq) → KCl (aq) + H⁺ (aq) + F⁻ (aq)

Explanation:

KF (aq) + HCl (aq) → KCl (aq) + HF (aq)

KF (aq) → K⁺ (aq) + F⁻ (aq)

HCl (aq) → H⁺ (aq) + Cl⁻ (aq)

KCl (aq) → K⁺ (aq) + Cl⁻ (aq)

HF (aq) → H⁺ (aq) + F⁻ (aq)

7 0

3 years ago

Define saturated and unsaturated fats

saul85 [17]

Answer:

SATURATED: Saturated fat is a type of fat in which the fatty acid chains have all or predominantly single bonds.

UNSATURATED: Unsaturated fats are loosely packed. They tend to be liquid at room temperature.

There are two main types of unsaturated fat:

Monounsaturated

Polyunsaturated

8 0

2 years ago

Which of the following are required for plants to carry out photosynthesis?

Vika [28.1K]

Answer:

Carbon dioxide, water, and sunlight

Explanation:

3 0

2 years ago

The enthalpy change for converting 1.00 mol of ice at -50.0 ∘c to water at 60.0∘c is ________ kj. the specific heats of ice, wat

guajiro [1.7K]

First, we have to get:

1- The heat required to increase T of ice from -50 to 0 °C:

according to q formula:

q1 = m*C*ΔT

when m is the mass of ice = mol * molar mass

= 1 mol * 18 mol/g

= 18 g

and C is the specific heat capacity of ice = 2.09 J/g-K

and ΔT change in temperature = 0- (-50) = 50°C

by substitution:

∴q1 = 18 g * 2.09 J/g-K *50°C

= 1881 J = 1.881 KJ

2- the heat required to melt this mass of ice is :

q2 = n*ΔHfus

when n is the number of moles of ice = 1 mol

and ΔHfus = 6.01 KJ/mol

by substitution:

q2 = 1 mol * 6.01 KJ/mol

= 6.01 KJ

3- the heat required to increase the water temperature from 0°C to 60 °C is:

q3 = m*C*ΔT

when m is the mass of water = 18 g

C is the specific heat capacity of water = 4.18 J/g-K

ΔT is the change of Temperature of water = 60°C - 0°C = 60°C

by substitution:

∴q3 = 18 g * 4.18 J/g-K * 60°C

= 4514 J = 4.514 KJ

∴the total change of enthalpy = q1+q2+q3

= 1.881 KJ +6.01 KJ + 4.514 KJ

= 12.405 KJ

5 0

3 years ago

Determine the number of molecules in a 100. gram sample of CCl4

enyata [817]

100. g CCl4* (1 mol CCl4/ 153.8 g CCl4)* (6.02*10^23 CCl4 molecules/ 1 mol CCl4)= 3.91*10^23 CCl4 molecules.
(Note that the units cancel out so you get the answer)

Hope this helps~

8 0

3 years ago