Agas of 19 ml at a pressure of 740 mmhg can be expected to change its pressure when its volume changes to 30. ml. express its new pressure in units of atmospheres.

To solve this we assume that the gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant temperature and number of moles of the gas the product of PV is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

P1V1 =P2V2

P2 = P1V1/V2

P2 = 740mmhg x 19 mL / 30 mL

P2 = 468.67 mmHg = 0.62 atm

your answer would be “dry”