Help please A gas in a sealed container has a pressure of 125 kPa at a temperature of 303K. If the temperature in the container is increased to 487K, what is the new pressure?

A 201kpa
B 200kpa
C 400kpa
D 78kpa​

A. 201 kPa

Explanation:

We can solve this problem by using Boyle's law, which states:

Where subscript 1 stands for the initial Pressure and Temperature, while 2 stands for the final conditions. That means that in this case:

We input the data:

And solve for P₂:

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.