Hello. If somebody has time can you check my answers? Q1: A gas occupies a 2.0L container at 25°C and 2.0atm. If the volume of the container is halved and the temperature remains constant, what is the new pressure? P1V1 = P2V2 P2 = 2.00 atm x (2.00L / 1.00L) = 4.00 atm --- Q2: The volume of 50mL of an ideal gas at STP increases to 100mL. If the pressure remains constant, what is the new temp? V1/T1 = V2/T2 T2 = (100mL / 50 mL) x 273K T2 = 546K --- Q3: How many moles of Oxygen gas, O2, are present in a 3.5L container held at a pressure of 0.5atm and a temp of 77°C? n = PV/RT n = (0.5atm x 3.5L) / (0.082 L•atm/mol•K x 350K) n = 50.225 mole O2 Thanks in advanced if you take the time to check these for me.