The molecular theory states that the pressure exerted by a gas in a closed vessel results from the gas molecule is striking against the walls of the vessel how will the pressure change if:
(a)the temperature is doubled keeping the volume constant
(b)the volume is made half of its original volume.
Asked by Abhishek | 4th Jan, 2018, 07:20: PM
Answered by Varsha | 4th Jan, 2018, 07:59: PM
- A container containing hydrogen gas is heated such that its volume increases by 40% and pressure decreases to 80% of its original value. If the original temperature was – 130C, calculate the temperature to which the gas was heated.
- A gas occupies a volume of 340 CC at STP find its volume at 20 degrees celsius and 700 mm of HG
- 100cm3 of a gas at 27°c is cooled to 20°c at constant pressure .calculate volume of a gas at 20°c
- A vessel of capacity 600 cm cube contains hydrogen gas at a pressure of 304 cm what will be the pressure of hydrogen gas when the vessel is connected to another vessel of 300 cm cube capacity
- It is found, on heating a gas, its volume increases by 50% and pressure decreases to 60% of its original value. If the original temperature was -15 degree celcius, find the temperature to which it was heated in celcius
- At constant temperature, a gas is at a pressure of 1080 mm Hg. If the volume is decreased by 40%, find the new pressure of gas
- a gas occupies 200 cm3 at 27 degree celsius. what is its volume at 51 degree celsius , the pressure being kept constant?
- Ammonia gas occupies volume of 450ml at a pressure of 720mm of HG what volume will it occupies at standard pressure at the same temperature
- A gas x occupies a volume of 200ml at a pressure of 4 atmospheres. If the temperature remains constant what volume will it occupy at 1atmospheric pressure
- I didn’t understood v vs 1/p graph
Kindly Sign up for a personalised experience
- Ask Study Doubts
- Sample Papers
- Past Year Papers
- Textbook Solutions
Verify mobile number
Enter the OTP sent to your number