A sample of a gas occupies a volume of 1100 mL at 78ºC and 0.060 atm. What would be the new volume if the temperature decreased to 44ºC and the pressure increased to 1.31 atm?

Md Ariful Islam

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Md Ariful Islam

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p1 = 0,06 atm = 6079,5Pa V1 = 1100ml = 0,0011m3 T1 = 780C = 351 K p2 = 1,31 atm = 132735,8Pa T2 = 440C = 317 K V2 - ? p1* V1 = m/M*R* T1 p2* V2 = m/M*R* T2 p1* V1 p2* V2 = T1 T2 V2 = p1* V1*T2 p2* T1 =6079,5Pa* 0,0011m3*317 K 132735,8Pa* 351 K = 4,5*10^-5 m3
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A sample of oxygen gas occupies a volume of 0.4652 L. When the volume is increased to 0.5782 L, the new pressure is 341.3 atm. What was the original pressure? Gas Law used :_______________

n= pV/RT = 341.3 x 0.5782/8.314 x 300 = 0,079119421.p=nRT/V= 0,079119421 x 8.314 x 300/0.4652 = 424,203912 atm.

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A sample of a gas occupies 250. mL at 1.00 atm of pressure. If the pressure increases to 2.00 atm while the temperature stays the same, what is the new volume?

P1V1 = P2V2P1 = 1V1 = 250 mlP2 = 2V2= ? 1×250 = 2V2 = 250/2V2 = 125 ml

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At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ?

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 =...

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A sample of carbon dioxide occupies a volume of 3.50 liters at 125 kPa pressure> What pressure would the gas exert if the volume was decreased to 2.00 liters?

According to the combined ideal gas equation:p1V1 = p2V2where p1 - initial pressure, V1 - initial volume, p2 - final pressure, V2 - final volume.From here:p2 = p1V1 / V2...

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A sample of carbon dioxide occupies a volume of 3.50 liters at pressure 125 kPa. What pressure would the gas exert if its volume was decreased to 1.75 liters?

 Boyle's Law can be expressed as  P1V1 = P2V2initial pressure P1 = 125 Kpainitial volume V1 = 3.50 Lfinal pressure P2= ??final volume V2 = 1.75 LHence P2 = P1V1/V2P2 = 125 KPa...

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