How do you solve a change in pressure question of a gas?
1. A 10.0-liter chamber contains a mixture of nitrogen and oxygen at a total pressure of 760 torr and a constant temperature of 25°C. The mole fraction of oxygen in the mixture is 0.211. a) Calculate the number of moles of oxygen in the chamber. ANSWER: 0.0862 moles O2 (oxygen gas) b) Gas is pumped out of the chamber until the total pressure is 0.100 torr. Calculate the new partial pressure of oxygen in the chamber. ANSWER: 2.77x10^-5 atm or .0211 torr O2 c) Pure nitrogen gas is added to the chamber until the total pressure is again 760 torr, then gas is pumped out of the chamber until the total pressure is 0.100 torr. Calculate the new partial pressure of oxygen after this process. how do i do part c above knowing what i know in the initial statement and knowing the answers to part a and b Thank you so much !
How to solve this question?
A high-pressure gas cylinder contains 40.0 L of toxic gas at a pressure of 1.60 x 10^7 N/m2 and a temperature of 27.0°C. Its valve leaks after the cylinder is dropped. The cylinder is cooled to dry ice temperatures (-78.5°C), to reduce the leak rate and pressure so that it can be safely repaired. (a) What is the final pressure in the tank, assuming a negligible amount of gas leaks while being cooled and that there is no phase change? N/m2 (b) What is the final pressure if one-tenth of the gas escapes? N/m2 (c) To what temperature must the tank be cooled to reduce the pressure to 1.00 atm (assuming the gas does not change phase and that there is no leakage during cooling)?
What is the final pressure of the gas? masteringphysics.com question?
PV = nRT ==> P = nRT/V = 0.67*8.314472*573.15/6E-5 = 5.3214E7 Pa EDIT: You don't have to solve for initial P at initial T as 2nd answer says, just solve for final P at final T.
Help with Chemisty Questions?! Solving Gas Law Problems?
1......CHARLES' LAW : 'The volume of a given mass of gas, is directly proportional to its absolute temperature, when its pressure remains constant' Volume Decrease <====> Temperature Decrease. Remember to use Kelvin temperature. (°C + 273 = K). (745mmHg / 775mmHg) x 303K = 291.3K - 273 = 18.3°C New temperature. 2.....BOYLE'S LAW: 'The volume of a given mass of gas, is inversely proportional to its absolute pressure, when its temperature remains constant ' P1V1 = P2V2 Pressure Increase <=====> Volume Decrease. (0.75atm / 2.35atm) x 10.0L = 3.2 L new volume.
A perfect gas at 27°C is heated at constant pressure till its volume is doubled. What will be its final temperature?
According to ideal gas equation PV=nRTP=pressure of gas,V=volume of gas=volume of container,T=temperaturueV1 =INITIAL VOLUME ,V2 =FINAL VOLUMET1 =INITIAL TEMPERATURE =27+273=300T2 =FINAL TEMPERATUREAccording to question,V2 =2 x V1Therefore,V1/V2 = T1/T2V1/2V1=300/T2T2 =FINAL TEMPERATURE=600KVidyanchal Academythank you
How do I solve this problem about work done on a gas being compressed?
Gas in a container expands at a constant pressure of 54 atm. Find the work done by the gas if the initial volume is 5 L and the final volume is 10 L . Answer in units of J. Alright, so for this problem I'm using this formula: W = PΔV (work = pressure * change in volume). I'm just wondering if I have these numbers plugged in correctly (and if I'm using the correct formula?). W = 54Pa * (10L - 5L) => W = 270J Thanks!