3. Elektron bergerak dalam daerah di antara 2 plat paralel dengan kecepatan 1.88 x 107 m/s dan melalui beda potensial 1000 V. Tentukan besar medan magnet agar elektron menempuh garis lurus. V₂ = 1000 V + + + + + + + + + + + +++ + X X X X X X X X X X X X X X X X X X X X X X X X X X X X X X V₁ = 0 V b 2 cm
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- Given R= 8.31 J mol·' K-' mol', k= 1.38 x10-23 J K-', NA = 6.23 x 10²3 mol- 1. Calculate a) the mean translational kinetic energy of carbon dioxide molecule with a relative molecular mass of 44 at 20 °C [ans: 6.07×10-21 J] b) the mean translational kinetic energy of a molecule on an ideal gas at 10 °C? [ans: 5.86×10-21 J]+ |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at a pressure of 0.340 bar, and the 2.50 L bulb contains oxygen (O,) at a pressure of 0.510 bar. 02 ON After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (CON) 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will remain constant. O There is not enough information to determine how the total pressure will change. O The total pressure will decrease. O The total pressure will increase. MacBook Pro ( The %23 %24 7. 4. 5. 3. R %3D K. H. B C. option command MOSISO181°F Which statement describes the overall relationship between volume and pressure? Esc O exponential O negative linear O direct O positive linear Partly sunny F2 -0- 2 F3 #M 3 F4 $ 4 F5 % 5 F6 Search -F7 6 F8 & 7 F9 * 8 F10 9 & 09 F11 S 1 0 F12 G Prt Sc
- Mg(s) + 2 HCl(aq) → MgCl2(g) + H2(g) PV = nRT R = 0.082061. 2. The volume of hydrogen gas produced was not at standard temperature and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure: STP (T = 273.15K and P = 1.00 atm). Mass of flask/stopper/5 mL H2O=112.794 g Mass of flask/stopper/filled flask of H2O=250.302 g Volume of gas space in flask (the difference between the above two measurements converted to L) =0.137508 L Trial 1: mass of Mg (g) =0.013 g pressure= 1.0104 atm temperature= 298.35 K moles of H2 =0.00054 molNitroglycerine ( C,H,N,O,) is a very strong explosive that degrades over time and is too shock sensitive to transport safely. Dynamite is made by combining nitroglycerine with stabilizers and adsorbents, which makes it much safer to use. The explosion of nitroglycerin can be represented by: 4 C,H,N,O,() → 6 N2(9) + 12 CO(9) + 10 H,0(9) + 7 O2(9) A stick of 40% dynamite is about 20 cm long and about 3 cm in diameter and weighs 241 grams. It is 40.0% nitroglycerine by mass. What is the total number of moles of gas produced when a stick of 4o% dynamite explodes? mol gasFe?+ + Ce*= Fe+ +Ce* which is described under normal conditions by the following parameters: E°A = E°re3+2+ = 0.771 (±0.005) V versus NHE; E°8 =Eos+3= 1.44 (± 0.02) V versus NHE; F = 96485.309 (± 0.029) C/mol (or J/ (V mol)). Calculate the AG° value for the Fe2*/Ce** reaction. Report your answer using the correct number of significant figures.
- If 400cm^3 of Q was collected at 25°c and 1.20 x10^5, calculate the volume it would occupy at s.t.p and the number of molecules of Q present.(standard pressure=1.0 x 10^5 Nm^-2 Avogadro's constant= 6.023 x 10^23, 1 mole of gas occupies 22.4 dm^3 at s.t.p)2 dN F (V )dV = N M 4 7 (- 2 ART MV 3/2y ? exp( 2 RT where dN, the number of particles having a velocity between v and v+dV, V velocity of molecules, M moleculer mass of gase, T temperature = |V ² † (V )dV =? 2-The data below is for a sample of gas at 25°C. Volume Difference in Hg Pressure Levels (mm) (mm x mL) 35.6 710 34.9 +15 33.7 +40 31.2 25.3 36.6 38.3 -50 41.4 50.6 -210 Now, calculate the P x V product (this is the proportionality constant, k) for each volume and pressure and fill in the column in the table. Complete the statements below: Statements: 1. The name of the curve you graphed is 2. The mathematical relationship between P and V is 3. The value of the proportionality constant, k, is. 4. The volume of this sample of gas at 2.00 atm and 25°C would be (Show your calculation in the space below.) 185
- 6. Using dimensional analysis, show how 0.082057 Latm mol. K Significant figures note: the last digit on both values has been rounded. NOTE: 1 J = 1 N-m = 1 kg.m², and 1 Pa = 1 N m² is equal to 8.3145 or 1 kg m.s mol - K4. A certain gas obeys the equation PVm = RT + a¡P + a¿P² where Vm is the molar volume, and a, and az are constants dependent only on the temperature. What will be the expressions for AF and A.1 when 1 mole of the gas is compressed from a pressure P, to a pressure P, at temperature T?The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles ( n): PV = nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b, which are unique to each substance: (P+ ²) (V-nb) = nRT an² The gas constant R is equal to 0.08206 L.atm/(K-mol). Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) mass of NH3 = Submit ▾ Part B HÅ…