1.) a 0.964 gram sample of a mixture of sodium formate andsodium chloride is ana

Question

1.) a 0.964 gram sample of a mixture of sodium formate andsodium chloride is analyzed by adding sulfuric acid. The equationfo the reaction for sodium formate with sulfuric acid is 2HCOONA +H2SO4 -> 2CO + 2H2O +Na2SO4. The carbon monoxide formed measures242 milliliters when collected over water at 752 torr and 22degrees Celsius. The partial pressure of water at 22 degreesCelsius is 19.8 torr. A.) Calculate the partial pressure of carbon monoxideproduced B.) Calculate the moles of carbon monoxide produced. C.) Calculate the percentage (by mass) of sodium formate inthe original mixture.
2.) GAS SAMPLE DATA Volume of sample: 90.0mL Temperature: 25 degrees Celsius Atmospheric Pressure: 745 mm Hg Equilibrium Vapor Pressure of H2O (25degreesCelsius): 23.8 mm Hg A student collected a sample of hydrogen gas by thedisplacement of water. A.) Calculate the number of moles of hydrogen gascollected B.) calculate the number of molecules of water vapor in thesample of gas.

3.) A rigid 5.00 L cylinder contains 24.5 g ofN2(g) and 28.0 g of O2(g) A.) Calculate the total pressure, in atm, of the gas mixturein the cylinder at 298 K. B.) The temperature of the gas mixture in the cylinder isdecreased to 280 K. Calculate the mole fraction of N2(g)in the cylinder. Also calculate the partial pressure, in atm, ofN2(g) in the cylinder. C.) If the cylinder develops a pinhole-sized leak and some ofthe gaseous mixtrue escapes, would the rationN2(g)/P2(g) in the cylinder increase,decrease, or remain the same? Justify and explain your answerplease. D.) a different rigid 5.00 L cylinder contains 0.176 mol ofNO(g) at 298K. A 0.176 mol sample of O2(g) is added tothe cylinder, where a reaction occurs to produceNO2(g). Write the balance equation for the reaction E.) Calculate the total pressure, in atm, in the cylinder at298 K after the reaction is complete.


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Explanation / Answer

question # 1 I answered for yoiu @ yahoo answers #2 PV=nRT (745 total - 23.8 H2O vapor Torr)(0.0900Litres) = n (62.4Torr-Litres/mol-K)(298K) n = 0.00349 moles of H2 B.) to calculate the number of molecules of water vapor, firstfind moles PV=nRT (745 total - 23.8 H2O vapor Torr)(0.0900Litres) = n (62.4Torr-Litres/mol-K)(298K) n = 0.00349 moles of H2 B.) to calculate the number of molecules of water vapor, firstfind moles (23.8 H2O vapor Torr)(0.0900Litres) = n (62.4Torr-Litres/mol-K)(298K) n = 0.000115 moles of H2O now, use avagadro's number to find molecules 0.000115 moles of H2O @ 6.02 e23 items /mole = 6.93 e19 molecules of water aka 6.93 X10 ^19 molecules ======================================================= 3.) A rigid 5.00 L cylinder contains 24.5 g ofN2(g) and 28.0 g of O2(g) A.) Calculate the total pressure, in atm, of the gas mixturein the cylinder at 298 K. use molar mass to find moles: 24.5 g N2 @ 28.0 g/mol = 0.875 mol N2 28.0 g O2 @ 32 g/mol = 0.875 mol O2 total moles = 1.75 moles of gas find pressure: PV = nRT atm (5.00L) = 1.75 mol(0.0821 L-atm/mol-K)(298K) pressure = 8.56 atm ====================== B.) The temperature of the gas mixture in the cylinder isdecreased to 280 K. Calculate the mole fraction of N2(g) in thecylinder. N2 has a mol fraction of 0.500 Also calculate the partial pressure, in atm, ofN2(g) in the cylinder @ 280 K knowing that N2 made up 1/2 of the pressure of 8.56 atm @298K... 4.28 atm P1 T2 = P2T1 (4.28atm)(280K) = P2(298K) P2 = 4.02 atm ======================================= C.) If the cylinder develops a pinhole-sized leak and some ofthe gaseous mixtrue escapes, would the rationN2(g)/P2(g) in the cylinder increase,decrease, or remain the same? Justify and explain your answerplease. I sure this was to mean: the ratio N2(g)/O2(g) By Grahams law, the N2 will escape faster, as its mass issmaller so the ratio N2(g)/O2(g)  will decrease ========================================= D.) a different rigid 5.00 L cylinder contains 0.176 mol ofNO(g) at 298K. A 0.176 mol sample of O2(g) is added tothe cylinder, where a reaction occurs to produceNO2(g). Write the balance equation for the reaction 2NO & O2 --> 2NO2 ================================ E.) Calculate the total pressure, in atm, in the cylinder at298 K after the reaction is complete. the moles @ the beginning was 0.352 at the end, 2 moles are produced while 3 are consumed so 2/3 's of 0.352 moles = 0.2347 moles are produced PV =nRT P(5.00L) = 0.2347mol(0.0821 L-atm/mol-K)(298K) P = 1.148 atm in a 3sig fig problem that rounds off to P = 1.15 atm ==================================== P.S. for me to answer your future chem problems... post as many as you wish, however... have fewer questions per posting, post them on yahoo answers, & email me of the posting as you did for the otherquestions po 3.) A rigid 5.00 L cylinder contains 24.5 g ofN2(g) and 28.0 g of O2(g) A.) Calculate the total pressure, in atm, of the gas mixturein the cylinder at 298 K. use molar mass to find moles: 24.5 g N2 @ 28.0 g/mol = 0.875 mol N2 28.0 g O2 @ 32 g/mol = 0.875 mol O2 total moles = 1.75 moles of gas find pressure: PV = nRT atm (5.00L) = 1.75 mol(0.0821 L-atm/mol-K)(298K) pressure = 8.56 atm ====================== B.) The temperature of the gas mixture in the cylinder isdecreased to 280 K. Calculate the mole fraction of N2(g) in thecylinder. N2 has a mol fraction of 0.500 Also calculate the partial pressure, in atm, ofN2(g) in the cylinder @ 280 K knowing that N2 made up 1/2 of the pressure of 8.56 atm @298K... 4.28 atm P1 T2 = P2T1 (4.28atm)(280K) = P2(298K) P2 = 4.02 atm ======================================= C.) If the cylinder develops a pinhole-sized leak and some ofthe gaseous mixtrue escapes, would the rationN2(g)/P2(g) in the cylinder increase,decrease, or remain the same? Justify and explain your answerplease. I sure this was to mean: the ratio N2(g)/O2(g) By Grahams law, the N2 will escape faster, as its mass issmaller so the ratio N2(g)/O2(g)  will decrease ========================================= D.) a different rigid 5.00 L cylinder contains 0.176 mol ofNO(g) at 298K. A 0.176 mol sample of O2(g) is added tothe cylinder, where a reaction occurs to produceNO2(g). Write the balance equation for the reaction 2NO & O2 --> 2NO2 ================================ E.) Calculate the total pressure, in atm, in the cylinder at298 K after the reaction is complete. the moles @ the beginning was 0.352 at the end, 2 moles are produced while 3 are consumed so 2/3 's of 0.352 moles = 0.2347 moles are produced PV =nRT P(5.00L) = 0.2347mol(0.0821 L-atm/mol-K)(298K) P = 1.148 atm in a 3sig fig problem that rounds off to P = 1.15 atm ==================================== P.S. for me to answer your future chem problems... post as many as you wish, however... have fewer questions per posting, post them on yahoo answers, & email me of the posting as you did for the otherquestions po

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