Given a 500 m sample of H#_2# at 2.00 atm pressure. What will be the volume when the pressure is changed to 720. torr? Chemistry Gases Gas Laws 1 Answer anor277 Jun 18, 2017 Well, #P_1V_1=P_2V_2#........so #V_2=1055.6*mL# Explanation: #V_2=(P_1V_1)/P_2# #=(2*atmxx500*mL)/((720*"Torr")/(760*"Torr"*"atm"^-1))=1055.6*mL#. Answer link Related questions How does Boyle's law relate to breathing? In Avogadro's Law what would happen to V if N is increased/decreased? And what would happen to n... How do you find the moles of a substance or the molecular formula with gas laws? Specifically,... What is Avogadro's Law? If you have 21 moles of gas held at a pressure of 78 ATM and a temperature of 900 k, what is the... If 57 moles of gas is held at a pressure of 5 atmospheres at a temperature of 100 Kelvin what... If gas occupies 56.44 L at 2.000 atm and 310.15 K. If the gas is compressed to 23.52 L and the... What does the R stand for in the ideal gas law (PV=nRT)? What is the mass of a gas that occupies 48.9 liters, has a pressure of 724 torr, a temperature... If a sample of neon gas occupies a volume of 2.8L at 1.8 atm. what will its volume be at 1.2 atm? See all questions in Gas Laws Impact of this question 1529 views around the world You can reuse this answer Creative Commons License