A gas exerts a pressure of 2.0 atm, at 30°C, in a 10 L container. In what size container would the same amount of gas exert a pressure of 4.0 atm at 20° C?

(2-0.7)=atm1.3atm

P1V1/T1 = P2V2/T2P1 = 1 atmV1 = 25 LT1 = 37+273 = 310KP2 = 1 atmV2 = 22 LT2 = ?= 1×25/310 = 21×1/X= 0.080645 = 21/X0.080645X = 21X =...

total pressure is 2 atmFlourine+.5 atmHydrogen=2.5 atmtotalremember that pH/ptot=nH/ntot=vh/vtot so the mole ratio of hydrogen to the mixture is is .5/2.5=.2 molHydrogen to 1 moltotal

P1V1= P2V2740×1= 2×V2740= 2V2V2= 740/2= 370mmHg

Presure exerted =1480mmHg

For answering this question you need to use the next law: PV = nRT V, R, n are constants P is pressure T is temperature From the first law: P1/T1...

As we know, Total pressure is the sum of partial pressure of individual gases.PT = 1.05 -(0.08+0.05+Pair)Pair = [0.92] atm

For this task we use the Dalton’s law which says that total pressure of mixture of gases equals to the sum of partial pressures of individual gases: Ptotal=PA+PB+PC+PD Therefore PD...

Answer on Question #83513Container A holds 782 mL of ideal gas at 2.80 atm. Container B holds 174 mL of ideal gas at 4.40 atm. If the gases are allowed...

P1 = P2 = 1.00 atm = constant;V1 = 22.4 L;T1 = 0 °C = 273.15 K;T2 = 95 °C = 368.15 K;V2 = unknown;Solution:(P1×V1)/(T1) = (P2×V2)/(T2);P1 = P2 =...