If the gas was collected at 40##^o## C and 75 mmHg then that is your initial condition. To find out what the volume is at any other condition you need to know what that condition is. You don't have enough information.Tasha Clifford said:
What are your thoughts on this so far? How many moles of gas are collected?Steve4Physics said:
I just edited the question now, it end with “STP” which i didnt write in capitals, does this mean STP conditions are the final conditionstopsquark said:
Brilliant, i think it makes much more sense nowSteve4Physics said:
Chestermiller said:
And Does this mean STP conditions of 273K andSteve4Physics said:
750 atm! Ouch!Tasha Clifford said:
First tell us what you think!Tasha Clifford said:
the number of moles is the same at both states.Tasha Clifford said:
I meant 75mmhg and notSteve4Physics said:
I do not quite understand what you mean here sirChestermiller said:
Maybe some confusion remains! Standard Temperature and Pressure (STP) corresponds to 0ºC and 750mmHg (but see note below).Tasha Clifford said:I meant 75mmhg and not750atmsorry for the mixup
You're certain?Steve4Physics said:
Yes. Post your working and answer and we'll check them.Tasha Clifford said:
Well (and you're probably going to explain why I'm wrong!) a quick Wikipedia check (https://en.wikipedia.org/wiki/Standard_temperature_and_pressure) doesn't disagree with what I wrote.Bystander said:
Steve4Physics said:
Who IS running the asylum these days?Maybe you mean that there are various definitions of STP (some using 750.06mmHg and others using 760mmHg)?Bystander said:
Note takenSteve4Physics said:
I don't really understand how i can solve this question using the ideal gas eqaution, i just tried and it’s giving me an absurd value, would appreciate if you can do so , i want to see how you go about itSteve4Physics said:
You need to show your working and the value you got.Tasha Clifford said:
The rules here require you to show evidence of your own work before we can offer guidance. See https://www.physicsforums.com/threads/homework-help-guidelines-for-students-and-helpers.686781/Tasha Clifford said:
The original question says that the initial pressure, P₁ = 75mmHg, not 750mmHg.Tasha Clifford said:
I am confused it’s actually an mcq qeustion, here is the questionSteve4Physics said:
I just did the necessary corrections and solved it solved it again but my answer still doesn't fall among the provided answersSteve4Physics said:
I agree with your answer. Well done! It looks like the question and/or answer-list have one or more mistakes. It happens sometimes.Tasha Clifford said:
Steve4Physics said:
##P_1V_1 = nRT_1##. Solve your initial condition to find the number of moles of the gas. Since this does not change, plug that into ##P_2 V_2 = nRT_2##.Tasha Clifford said:
Oktopsquark said:
Please how did you type the equation , i see it as( ##P_1V_1 = nRT_1##)topsquark said:
According to Charles' Law, as temperature increases, the volume of gas also increases, causing an increase in pressure. This is because the molecules in the gas have more energy and move faster, colliding more frequently with the walls of their container.
Boyle's Law states that as the volume of a gas decreases, the pressure increases, and vice versa. This is because a decrease in volume means the gas molecules have less space to move around, causing more collisions with the container walls and thus an increase in pressure.
According to the Combined Gas Law, as both volume and temperature increase, the pressure also increases. This is because the increase in volume allows more space for the gas molecules to move around, while the increase in temperature causes them to move faster and collide more frequently with the container walls.
The ideal gas law, PV = nRT, can be used to calculate the new pressure of a gas when volume and temperature are changed. By plugging in the initial values and solving for the new pressure, you can determine the new pressure of the gas after the changes.
According to Boyle's Law, pressure and volume have an inverse relationship in a gas. As one increases, the other decreases, and vice versa. This is because the number of gas molecules and temperature remain constant, so a change in volume will result in a change in pressure and vice versa.
