1. A fixed amount of gas at 20 degrees Celsius occupies a volume of12.0L under p

Question

1. A fixed amount of gas at 20 degrees Celsius occupies a volume of12.0L under pressure of 650 torr. Calculate its volume at the samepressure when the temperature is increased to 280 degrees Celsius.

2. Calculate the root-mean-square speed in m/s of CO2 gas inat 50 degrees Celsius
3.What is the density of chlorine gas (Cl2) in g/L at 850.00mm HG and 35 degrees Celsius
4. Zinc reacts with aqueous sulfuric acid to formhydrogen gas: Zn(s) + H2SO4(aq)-------> ZnSO4(aq) +H2(g) How many grams of zinc are required to generate 45.0L ofH2 gas at 1.2 atm and 22.0 degrees Celsius?

2. Calculate the root-mean-square speed in m/s of CO2 gas inat 50 degrees Celsius
3.What is the density of chlorine gas (Cl2) in g/L at 850.00mm HG and 35 degrees Celsius
4. Zinc reacts with aqueous sulfuric acid to formhydrogen gas: Zn(s) + H2SO4(aq)-------> ZnSO4(aq) +H2(g) How many grams of zinc are required to generate 45.0L ofH2 gas at 1.2 atm and 22.0 degrees Celsius?

Explanation / Answer

1. A fixed amount of gas at 20 degrees Celsius occupies avolume of 12.0L under pressure of 650 torr. Calculate its volume atthe same pressure when the temperature is increased to 280 degreesCelsius According to gas law PV = nRT Since Pressure kert constant , V T So V / V' = T /T'                     V& V' are initial & finalVolumes              T & T' are initial & final Temperatures V' = VT' / T      = ( 12L * (280+273)K ) / (20+273)     = 22.648 L 2.. Calculate the root-mean-square speed in m/s of CO2 gas inat 50 degrees Celsius r = ( 3RT /M) M = Molar mass of CO2 = 12 + 2 * 16 = 44 g/mol = 44*10^-3 Kg /mol R = gas constant = 8.314 J / mol - K T = Temperature = 50+273 = 323K So r = 427.89 m /s 3.What is the density of chlorine gas (Cl2) in g/L at 850.00mm HG and 35 degrees Celsius we know that P = dRT /M P = pressure = 850 mm Hg = 850/760 atm = 1.118 atm T = temperature = 35+273 = 308 K d = density = ? M = Molar mass of Cl2 = 71 g / mol R = gas constanyt = 0.0821 L atm / mol - K So d = PM/RT         = 3.1391 g /L 4. Zinc reacts with aqueous sulfuric acid to formhydrogen gas: Zn(s) + H2SO4(aq)-------> ZnSO4(aq) +H2(g) How many grams of zinc are required to generate 45.0L ofH2 gas at 1.2 atm and 22.0 degrees Celsius? PV = nRT        = ( m / M ) RT So , mass of H2 , m = PVM / RT                                 =(1.2 atm * 45 L * 2g/mol ) / ( 0.0821 L atm / mol - K * 295 K)                                = 4.4592 g of H2 according to the Equation, 65.38 g of Zn liberate 2 g of H2 X g of Zn liberate 4.4592 g of H2 X = ( 65.38* 4.4592 ) / 2     = 145.77 g of Zn Zn(s) + H2SO4(aq)-------> ZnSO4(aq) +H2(g) How many grams of zinc are required to generate 45.0L ofH2 gas at 1.2 atm and 22.0 degrees Celsius? PV = nRT        = ( m / M ) RT So , mass of H2 , m = PVM / RT                                 =(1.2 atm * 45 L * 2g/mol ) / ( 0.0821 L atm / mol - K * 295 K)                                = 4.4592 g of H2 according to the Equation, 65.38 g of Zn liberate 2 g of H2 X g of Zn liberate 4.4592 g of H2 X = ( 65.38* 4.4592 ) / 2     = 145.77 g of Zn        

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