20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3?
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
a.|A skydiver jumps out of an airplane and falls to the ground with increasing speed.| b.|A truck travels a twisty highway ranging from 40 km/h to 70 km/h.| c.|A horse trots around a circular track at a constant speed.| d.|A car travels down a straight highway at a steady 95 km/h.| ____ 9. How do you determine acceleration from an acceleration–time graph? a.|Read information from the graph.| b.|Find the area.| c.|Take the slope.| d.|none of the above|
EXPERIMENT 11 Molar Mass of a Volatile Liquid DATA Run | UNKNOW | Mass of flask and foil(g) | 90.085g | Mass of flask and foil and condensed vapor (g) | 90.640g | Temperature of boiling water (˚C ) | 98˚C | Barometric pressure (torr) | 761mm Hg | Volume of flask (mL) | 140 mL | RESULTS Mass of unknown ( condensed vapor) | 0.555g | Volume of flask (vapor)(L) | 0.14 L | Temperature of vapor(k) | 371K | Molar mass of unknown (g/mole) | 118.380 g/mole | Advance Study Assignment 1) How would each of the following errors affect the outcome of this experiment? Would it make the molar mass high or low? Give your reasoning in three sentences or less in each case. a) The hole in the aluminum foil was quite large. if you were to have a larger hole in your aluminum cap, you would be losing vapor to the room.
o D. The mass is not exactly 255.0 grams, but it is impossible to tell whether the mass is greater than or less than 255.0 grams. 5. 5. You place a mass of 250 grams on the measurement tray of a triple beam balance and then set the rider on the 500 gram beam to the 200 gram mark (the other riders are set to 0 grams). Which of the following statements is true?
If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium. 2 HI (g) === H2 (g) + I2 (g) Ke = 1.84(10-2 [H2]=[I2]= 1.07(10-2 mol/L, [HI]=7.86(10-2 mol/L 6. A 1.00 L reaction vessel initially contains 9.28(10-3 moles of H2S. At equilibrium, the concentration of H2S of 7.06(10-3 mol/L. Calculate the value of Ke for this system.
How many kilograms of pure HCl would be used to make this hydrochloric acid? (Assume that 30% has two significant figures. There are 2000 lb/ton.) (Obj 15) 30 ton HCl 2000 lb 1 kg ? kg HCl = 6.0 × 105 ton HCl soln 100 ton HCl soln 1 ton 2.205 lb 30 ton HCl 2000 lb 453.6 g 1 kg ?
mass = _____S_______________ 3. speed = ______S______________ 4. displacement = __V___________ 5. length = ____S_______________ Objective Four: Make and interpret position-time graphs that are equivalent representations that diagram an object’s uniform motion. Directions: Answer the following questions in the space provided. 1.) The graph to the right shows the distance versus time for two cars traveling on a straight highway. a.
k. RPM. The RPM limit is 6800. l. Transaxle. The Racecar’s transaxle is a racing five-speed plus reverse. m. Transmission. The Seller had the transmission last serviced by Taylor in 2009. n. Ownership.
How many multiple bonds (double and/or triple) are there in this molecule? (1 point for each molecule) There are no double or triple bonds on this molecule. CO2 4+2(6)=16 .. .. O = C = O .. .. 1. What is the central atom? (1 point for each molecule) The central atom is C. 2.