The pressure on a sample of an ideal gas is increased from 715 mmHg to 3.55 atm at constant temperature. If the initial volume of the gas is 485 mL, what is the final volume of the gas? Chemistry Gases Gas Laws 1 Answer anor277 · Meave60 Nov 28, 2016 Answer: The gas is compressed to a volume of #129*mL#. Explanation: At constant #T#, #P_1V_1=P_2V_2#; this is Boyle's law. Now #P_1=(715*mm*Hg)/(760*mm*Hg*atm^-1)=0.941*atm# #V_2=(P_1V_1)/P_2=(0.941*cancel(atm)xx485*mL)/(3.55*cancel(atm))=129*mL# 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 if ... How do you find the moles of a substance or the molecular formula with gas laws? Specifically, how ... 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 of ... 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 3074 views around the world You can reuse this answer Creative Commons License