The density of H₂ gas in a rigid container is 0.117 g/L at 55 $\circ$ C.What is the pressure of hydrogen in the flask if it is heated to 125 $\circ$ C? (R = 0.08206 L.atm/mol.K) A) 0.142 atm B) 0.194 atm C) 1.56 atm D) 1.90 atm E) 3.55 atm

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First, we need to use the ideal gas law to find the initial number of moles of H₂ gas in the container: PV = nRT 0.117 g/L = n(0.08206 L*atm/mol*K)(55+273 K) n = 0.0047 mol Next, we can use the combined gas law to find the new pressure at 125 F1F1F1S1F1F1F10C: (P1/T1) = (P2/T2) P2 = P1(T2/T1) P2 = (0.117 g/L)(0.08206 L*atm/mol*K)(398 K)/(0.0047 mol)(328 K) P2 = 1.90 atm Therefore, the answer is D) 1.90 atm.

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The Density of H₂ Gas in a Rigid Container Is $\circ$