(3.9) What is the density (in g/mL) of NH3 (g) at 10.0 °C and 1.15 atm? See notes below to solve for density, r. Atomic mass: N 14.007 H 1.008 Analysis (Given): Molar mass of NH3 = g/mol Temperature of NH3 = K Answer: density, r (NH3) = g/L (3 sig fig)
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- Fill in the blanks: (3.8) What volume (in mL) will 10.0 g of CO2 (g) Occupy at 27 °C and 2.00 atm? Atomic mass: C 12.01 O 16.00 Analysis (Given): T (CO2) = | K n mol (CO2) = %3D moL (3 sig fig) Answer: V (CO2) = mL %3D (3 sig fig)5. (8) A small bubble rises from the bottom of a lake, where the temperature and pressure are 7°C and 2.8 atm, to the water's surface, where the temperature is 27°C and pressure is 740 mmHg. Calculate the final volume in mL. of the bubble if it's initial volume was 1.5 mL.(706 mmHg = latm)(7.50ml) Charles' Law 1. Several balloons are inflated with helium to a volume of 0.75 L at 27°C. One of the balloons was found several hours later, the temperature had dropped to 22°C. What would be the volume of the balloon when found, if no helium has escaped? (0.74L) Sign out V 8 12 DELL %23 %24 & 4 6 [O e r t y u d. f m alt ctri of
- 6. V₁6.00L P₁=730 P₂=760, (760.) (.) Calculate the final pressure inside a scuba tank after it cools from 1.00 x 10³ °C to 25.0 °C. The initial pressure in the tank is 130.0 atm. (6.00, 7. A sample of ammonia has a volume of 60.0 mL at 0°C. At what temperature will it have a volume of 325 mL? 60 77731(6.9: Similar to Example 6.15 & For Practice 6.15) Find the ratio of effusion rates of argon gas and chlorine gas. O 0.751 O 1.33 O 3.15 O 0.317(6.7: Similar to For practice 6.12)In the reaction shown here, 955 mL of O2 forms at P = 0.950 atm and T-308 K. How many grams of Ag2O (molar mass = 231.8 g/mol) decomposed? 2Ag2O(s) --> 4 Ag(s) + O2(g) O 1.15 g O 0.574 g O 8.32 g O 16.6 g
- PV=nRT R= 0.0821 atmL/molK Molar Mass of H, = 2 g/mol. Ammonium sulfate, (NH,),SO, is an important fertilizer and can be prepared by the reaction of ammonia (NH,) with sulfuric acid (H,SO,) according to the following balanced equation: 2 NH, + H,SO, (NH,),SO, 11. a. Calculate the moles of NH, needed to react with 0.35L of a 1.25 M H, SO, solution. b. How many liters of NH, gas are needed if the pressure is 0.9 atm and the temperature is 266 K? (NOTE: You will need your answer from part a to calculate this answer)11.114 2.00 L of N,, at 25 °C and 1.08 atm, is mixed with 4.00 I of O2, at 25 °C and 0.118 atm, and the mixture is allowed to react. How much NO, in grams, is produced? (9.2, 9.3, 11.7, 11.8) N2(g) + O2(8) → 2NO(8)Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH3CO₂(aq) + C₂H²OH(aq) → C₂H₂CO₂CH₂(aq)+H₂O(1) Imagine 230. mmol of C₂H²CO₂CH3 are removed from a flask containing a mixture of HCH³CO₂, C₂H²OH, C₂H²CO₂CH3 and H₂O at equilibrium, and then answer the following questions. What is the rate of the reverse reaction before any C₂H5CO₂CH3 has been removed from the flask? What is the rate of the reverse reaction just after the C₂H5CO₂CH3 has been removed from the flask? What is the rate of the reverse reaction when the system has again reached equilibrium? How much less C₂H5CO₂CH3 is in the flask when the system has again reached equilibrium? O O O O O O O O O O O O O O O O Zero. Greater than zero, but less than the rate of the forward reaction. Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. Zero. Greater than zero, but less than the rate of the forward reaction. Greater than…
- 4 4 2$ 8. 7. 9. 6. IIO | other one? Latm/mol.K. Use the total mol to find mol of each gas. Let x = one of the gases.What's the mass of the Hint: Find n using the ideal gas la, making sure that T is in K, P is in atm, V is in L and R = 0.08206 %3D 870.2 mmHg and 31.2°C. What is the mole fraction of nitrogen in this mixture? A 26.5-g mixture of nitrogen and carbon dioxide is found to occupy a volume of 16.5 L when measured atof F. Hydrazine, N,H, reacts with oxygen to form nitrogen gas and water. If 3.75 g of N,H, reacts with excess oxygen and produces 0.750 L of N, , at 295 K and 1.00 atm, what is the percent yield of (DOʻHT + (3)°N – (3)°0 + (be)*H’N the reaction? percent yield: MacBook Pro & 4. 9. 7. 6. P. H. K. B M. N17. A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetraoxide (N2O4), which ignite on contact to form nitrogen gas and water vapor. How much in grams of the excess reagent is used up when 435.0 g of N2H4 and 718.5 g of N2O4 are mixed? (, MW: N204 = 92.011g/mol, N2H4 = 32.05g/mol, N2 =28.013 g/mol 2N2H4(0) + N2O40) –> 3N2(9) + 4H2O(g)