Question

The volume of a fixed amount of gas is doubled, and the absolute temperature is doubled. According to the ideal gas law, how

has the pressure of the gas changed?
It has increased to two times its original value.
It has increased to four times its original value
It has decreased to one-half its original value.
It has stayed the same.

Answer 1

D

Step-by-step explanation:

im taking the final rn too

Answer 2

Option D is correct: It has stayed the same.

Step-by-step explanation:

Data Given:

fixed amount of gas

volume = 2x

Absolute temperature = 2x

effect on Pressure according to ideal gas law.

Solution:

To know the effect we will made calculation by ideal gas law

As,

we know that pressure for ideal gas law = 1 atm

Now we look for this change in pressure from 1 atm

new pressure can be calculated by using ideal gas formula

PV = nRT

Rearrange the equation for Pressure

P = nRT / V . . . . . . . . . (1)

where

P = pressure

V = Volume

T= Temperature

n = Number of moles

R = ideal gas constant

Standard values

T = 273 K and its double will be

• T= 2 (273 K) = 546 K

Fixed amount of gas

• n = 1 mole

R = 0.08206 L.atm / mol. K

V = 22.42 L/mol and its double will be

V = 2(22.42 L/mol) = 44.84 L/mol

Now put the value in formula (1) to calculate Pressure

P = 1 x 546 K x 0.08206 L.atm/mol.K / 44.84 L/mol

P = 44.772 L.atm/mol / 44.84 L/mol

P = 0.9996 atm

So,

P ≅ 1 atm

It means there is no change in the pressure by double amount of temperature and volume.

Option D is correct. It has stayed the same.