Calculate the pressure, in atmospheres, of 2.0 mol of helium gas in a 10.0 L container at 27 degrees Celsius.

The pressure, in atmospheres, of the helium gas is 4.93 atm

From the question,

We are to determine the pressure of the helium gas

Using the formula

PV = nRT

Where P is the pressure

V is the volume

n is the number of moles

R is the gas constant

and T is the temperature

Then, we can write that

From the given information

n = 2.0 mol

V = 10.0 L

T = 27 °C = 27 + 273.15 K = 300.15K

and

R = 0.08206 L atm mol⁻¹ K⁻¹

Putting the parameters into the formula, we get

∴ P = 4.9260618 atm

P ≅ 4.93 atm

Hence, the pressure, in atmospheres, of the helium gas is 4.93 atm

Learn more here: link

4.92atm

Explanation:

From the question, the following were obtained:

V = 10L

T = 27°C = 27 + 273 = 300K

n = 2moles

R = 0.082atm.L/K /mol

P =?

Using the ideal gas equation PV = nRT, we can solve for the pressure as follows:

PV = nRT

P = nRT / V

P = (2x0.082x300) / 10

P = 4.92atm

a plasma is a warm ionized gasoline consisting of approximately equal numbers of definitely charged ions and negatively charged electrons. the characteristics of plasmas are notably unique from the ones of ordinary neutral gases in order that plasmas are considered a awesome "fourth kingdom of remember."

give me abc and i will get it for u.