A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90 moles of a gas(n1),?
Apply the Ideal Gas Law : --------------------------------------... ( P1 ) ( V1 ) = ( n1 ) ( R ) ( T1 ) ( P2 ) ( V2 ) = ( n2 ) ( R ) ( T2 ) For P2 = P1 and T2 = T1 : n1 / V1 = n2 / V2 V2 = ( V1 ) ( n2 / n1 ) V2 = ( 46.0 ) ( 1.4 / 1.9 ) = 33.9 L <---------------------------------------...
A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90 moles of a gas (n1), and?
A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90 moles of a gas (n1), and its volume is 45.0 L (V1). If 0.600 moles of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder?
A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90moles of a gas (n1), and?
Extremely stumped on this one! PART A: A cylinder, with a piston pressing down with a constant pressure, is filled with 1.90moles of a gas (n1), and its volume is 43.0L (V1). If 0.800mole of gas leak out, and the pressure and temperature remain the same, what is the final volume of the gas inside the cylinder? PART B: A sample of gas in a cylinder as in the example in Part A has an initial volume of 40.0L , and you have determined that it contains 2.00moles of gas. The next day you notice that some of the gas has leaked out. The pressure and temperature remain the same, but the volume has changed to 10.0L . How many moles of gas (n2) remain in the cylinder?
A sample of gas in a cylinder as in the example in Part A has an initial volume of 52.0 L, and you have determ?
V1 / n1 = V2 / n2 at constant pressure and temperature (52.0 L) / (2 mol) = (13.0 L) / n2 n2 = (13.0 L) (2 mol) / (52.0 L) n2 = 0.5 moles of gas For the second question: V1 / n1 = V2 / n2 at constant pressure and temperature (49.0 L) / (2.2 mol) = (V2) / (1.5 mol) V2 = (49.0 L) (1.5 mol) / (2.2 mol) V2 = 33.4 L Hope this helps...good luck!