Chapter 7a D2L Homework

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Chemistry

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Dec 6, 2023

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1 Chapter 7a D2L Homework Problems Name: __________Lamarla Fletcher_________ Please type or write your name on first page. If equations do not appear with older version of Word, use the PDF file format for this homework. 1. If a 224 gram block of dry ice, CO 2 , is sublimed at 45 C and 760. mm Hg of atmospheric pressure, what volume does the gas occupy? Write the calculated numerical value between the equal signs (=) and given units grams, mole, Kelvin, atmosphere and Liter. Calculate the molar mass of CO 2 Using atomic weights rounded off to 3 significant figures obtained from the Periodic Table 1 C atom = 12.0 and 2 O atoms = 2×16.0 Calculatemolar massof CO 2 = 12.0 + ( 2 × 16.0 ) = 44.0 gramsC O 2 1 moleC O 2 ( 3 sig .fig. ) Calculate the number of moles of CO 2 Number of molesof CO 2 = 224 gCO 2 × 1 moleC O 2 44.0 gCO 2 = 5.09 moleC O 2 ( 3 sig .fig. ) Calculate the temperature in Kelvin T K = 45 0 C + 273 = 318 K ( 3 significant figures ) Calculate the pressure in atmosphere: P = 760. mm Hg× 1 atm 760 mm Hg = 1.00 atm ( 3 signifcant figures ) Calculate the volume of 224 grams of CO 2 gas at 45ºC and 760. mm Hg pressure using the ideal gas law. IdealGas Law PV = nRT V = nRT P = 5.09 mol× ( 0.0821 Latm mol K ) × 318 K 1.00 atm = 298 L ( 3 sig .fig. )
2 Chapter 7a D2L Homework Problems Name: _________________________________ 2. The gas in aerosol can is at a pressure of 5.00 atmospheres at 25 C. What will the pressure be of the gas in the can if the temperature is raised to 650. C? Write the calculated numerical value between the equal signs (=) and unit Kelvin atmosphere. Use the ideal gas law for constant number n of moles of gas and constant volume V . Using the ideal gas law PV = nRT With n and V constant P T = nR V = Constant Value Therefore P 1 T 1 = P 2 T 2 T 1 P 1 = T 2 P 2 sinceif a = bthen 1 a = 1 b Calculate T 1 and T 2 in Kelvin T 1 = 25 0 C + 273 = 298 K ( 3 significant figures ) T 2 = 650 . 0 C + 273 = 923 K ( 3 significant figures ) And so P 2 = P 1 T 2 T 1 = 5.00 atm× 923 K 298 K = 15.5 atm ( 3 significant figures )
3 Chapter 7a D2L Homework Problems Name: _________________________________ 3. Arrange the following compounds in order of increasing expected melting points: Ne, NH 3 , CF 4 , MgO, NaOH, H 2 O, and C 6 H 12 O 6. Use Google Search to order these compounds from lowest to highest melting point at one atmosphere of pressure.
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4 Chapter 7a D2L Homework Problems Name: _________________________________ 4. A 10.0 Liter gas cylinder is filled with N 2 to a pressure of 75.0 atmospheres. How many moles of N 2 does one have to add to raise the pressure to 125 atmospheres? Assume a constant temperature of 25 C. Write the calculated numerical value between the equal signs (=) and unit Kelvin and mole. Use ideal gas law to calculate the number n 1 of moles of N 2 in a 10.0 Liter gas container at 25ºC and 75.0 atmospheres. Idealgaslaw PV = nRT Calculate temperature T in Kelvin scale T K = 25 0 C + 273 = K ( 3 significant figures ) Calculate number n 1 of moles of N 2 in a 10.0 Liter gas container at 25ºC and 75.0 atmospheres. n 1 = P 1 V RT = 75.0 atm× 10.0 L 0.0821 Latm mol K × 298 K = N 2 mole ( 3 sig .fig. ) Note constant volume V and constant temperature T so by the ideal gas law P n = RT V = Constant Value So from using the ideal gas law at constant V and constant T P 1 n 1 = P 2 n 2 n 1 P 1 = n 2 P 2 sinceif a = bthen 1 a = 1 b Calculate the number n 2 moles of N 2 gas at 125 atmospheres of pressure in 10.0 Liter at 25ºC n 2 = n 1 P 2 P 1 = 30.7 N 2 mole× 125 atm 75.0 atm = mole N 2 ( 3 sig.fig. ) The number of moles Δ n added to the 10.0 Liter container at 25ºC is the following difference.
5 ∆n = n 2 n 2 = 51.2 mole N 2 30.7 mole N 2 = mole N 2 ( 3 sig .fig. ) Chapter 7a D2L Homework Problems Name: _________________________________ 5. If the density of a gas is 0.0151 g/mL at 150. C and 1.50 atmospheres, what is the mass of one mole of the gas? Write the calculated numerical value between equal signs (=) and unit gram, Kelvin and mole. Use a gas volume V equal to 1.000 Liters or 1000. Milliliters Calculate mass of gas in 1000. Milliliters M = DV = 0.0151 g mL × 1000. mL = g ( 3 significant figures ) Calculate the temperature in the Kelvin scale T K = 150 . 0 C + 273 = K ( 3 significant figures ) Use the ideal gas law, PV = nRT , to calculate the number of moles of gas in 1.000 Liter at 150.ºC 1.50 atmospheres n = PV RT = 1.50 atm× 1.000 L 0.0821 Latm mole K × 423 K = mole ( 3 significant figures ) Now one can calculate the molar mass in units of grams per mole or the magnitude of the molecular weight MW MW = 15.1 g 0.0432 mole = grams 1 mole ( 3 significant figures )