When `2g` of gas `A` is introduced into an evacuated flask kept at `25^(@)C` the presusre is found to be `1atm`. If `3g` of another gas `B` is then added to the same flask the total pressure becomes `1.5 atm`. The ratio of

When 2 g of a gas A is introduced into an evacuated flask kept at 25^(@)C , the pressure is found to be 1 atm . If 3 g of another gas B is then heated in the same flask, the total pressure becomes 1.5 atm . Assuming ideal gas behaviour, calculate the ratio of the molecular weights M_(A) and M_(B) .

When 2 g of a gas A is introduced into an evacuated flask kept at 25^(@)C , the pressure is found to be 1 atm . If 3 g of another gas B is then heated in the same flask, the total pressure becomes 1.5 atm . Assuming ideal gas behaviour, calculate the ratio of the molecular weights M_(A) and M_(B) .

When 2g of a gas A is introduced into an evacuated flask kept at 25^@C , the pressure is found to be one atmosphere. If 3 g of another gas B are then added to the same flask, the total pressure becomes 1.5 atm. Assuming ideal gas behaviour, calculate the ratio of molecular weights M_A : M_B .

When 2g of a gas A is introduced into an evacuated flask kept at 25°C, the pressure is found to be 1 atmosphere. If 3g of another gas is then added to the same flask, the total pressure becomes 1.5 atm. Assuming ideal behaviour, the ratio of their molecular weights M_(A): M_(B) is

When 4 g of an ideal gas A is introduced into an evacuated flask kept at 25^(@)C , the pressure is found to be one atmosphere. If 6 g of another ideal gas B is then added to the same flask, the pressure becomes 2 atm at same temperature. The ratio of molecular weights (M_(A) : M_(B)) of the two gases would be