Pressure of 1 g ideal gas X at 300 K is 2 atm. When 2 g of another gas Y is introduced in the same vessel at same temperature, the pressure become 3 atm. The correct relationship between molar mass of X and Y is :
Pressure of 1 g of an ideal gas A at 27^(@)C is found to be 2 bar, when 2 g of another gas B is introduced in the same flask at same temperature. The pressure becomes 3 bar. Find a relationship between their molecular masses.
The presence of 1 g of an ideal gas A at 27^(@)C is 2 bar . When 2 g of another ideal gas B is added to the same flask at the same temperature, the pressure becomes 3 bar . The relationship between their molar masses is
Pressure of 1g of an ideal gas A at 27^(@)C is found to be 2 bar when 2g of another ideal gas B is introduced in the same flask at same temperature the pressure becomes 3 bar. Find a relationship thieir molecular masses .
The pressure of gas at 100^(@)C is 2 atm. When the gas is heated at constant volume. At what temperature the pressure raises to 3 atm?
A vessel of "50L" contains "40g" of an ideal gas "X" at "600K" .The pressure exerted by the gas is 1 atm."20g" of an ideal gas "Y" is added to the same vessel keeping the same temperature.Total pressure becomes "3atm" .If the molar mass of "gas X" is "m (g/mol)" and the molar mass of gas "Y" is "n (g/mol)" then find the value of "(m+n)" .(Use "R=(1)/(12)(atmL)/(molK)" )
16 g of O_(2) gas and x g of H_(2) occupy the same volume at the same temperature and pressure. Then x =
