QUESTION 10 If SL of wet O2 is collected over water at 25°C and a barometric pressure of 800 Torr, how many moles of O2 are present? O 14 0 14 O 14 O 140 QUESTION 11 A mixture of hydrogen (2 01 g) and chlorine (17.73 g) in a container at 300 K has a total gas pressure of 98.8 kPa What is the partial pressure of hydrogen in the mixture? O 794 kPa O 794 kPa O704 IPa O 7,940 kPa QUESTION 12 What is a polymor that forms by simple linking of monomers without the co-generation of other products O Addition Polymers O Polymers O Dehydration Polymers O Condensation Polymers

QUESTION 10 If SL of wet O2 is collected over water at 25°C and a barometric pressure of 800 Torr, how many moles of O2 are present? O 14 0 14 O 14 O 140 QUESTION 11 A mixture of hydrogen (2 01 g) and chlorine (17.73 g) in a container at 300 K has a total gas pressure of 98.8 kPa What is the partial pressure of hydrogen in the mixture? O 794 kPa O 794 kPa O704 IPa O 7,940 kPa QUESTION 12 What is a polymor that forms by simple linking of monomers without the co-generation of other products O Addition Polymers O Polymers O Dehydration Polymers O Condensation Polymers

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.25P: 5-25 A gas in a bulb as in Figure 5-3 registers a pressure of 833 mm Hg in the manometer in which...

See similar textbooks

Similar questions

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 94.6 g He and 48.5 g CO2 at 398K? 1 atm = 760 torr (exactly); R = 0.08206 L-atm/K-mol Question 19 options: 46.6 atm 81.0 atm 467 atm 50.6 atm 24.8 atm
Balanced Equation: Zn + 2HCl → ZnCl2 + H2 Net Ionic Equation: Zn + 2H → Zn2+ + H2 1. If a 0.25 g sample of Zn reacts with excess HCl… How many moles of HCl will react? How many moles of H2(g) should be produced? 2. The experiment takes place under the following conditions: 300 K, Patm = 777 mmHg, PH2O at 300 K = 26.7 mmHg. How many liters of H2 would be generated under these conditions from the reaction of 0.25 g Zn with excess HCl? 3. How would the amount of H2 collected change if the piece of zinc that reacted had a mass of 0.35 g? Explain.
What pressure (in atm) would be exerted by a mixture of 1.4 g of Chlorine gas (Mm= 70 g/mol) and 4.8 g of nitrogen gas (Mm= 28 g/mole) in a 200 mL container at 57oC? a. 4.7b. 34c. 47d. 26e. 0.030f. Option 6
Answer the following: 3. Beef is cooked in a pressure cooker with an initial pressure of 1.5 atm at 110 °C. If the volume is held constant, what will be the pressure inside the cooker if the temperature increases to 120 °C 4. A sample of a gas occupies 5.0 L at STP. What will the volume be if the temperature is set to 320 Kat a pressure of 1.2 atm? 5. If gas C effuses twice as fast as SO2, what is the molecular weight of gas C?
QUESTION 10 Small amounts of oxygen can be generated by the thermal decomposition of KClO 3; 2 KClO 3(s) ↔ 2 KCl(s) + 3 O 2(g) A sample of KClO 3 was decomposed and oxygen collected over water at 14.00 °C (Vapor pressure = 11.99 torr). How many liters would be collected if 2.631 g of KClO 3 decomposed and the gas was collected at 304.3 torr? Key Concept:Gases and reactions over water. Strategy: Reactants always react in a proportionate way. One can determine the mole of gases involved from the stoichiometry in the balanced reaction. Remember when you collect the gas over water you must subtract it's contribution from the total pressure of the gases in the collection device.
1. Many laboratory gases are sold in steel cylinders with a volume of 43.8 L. If there are x kilograms of argon inside a cylinder whose pressure is 4,592 kPa at 46°C, what the value of x? (1 atm = 101325 Pa) 2. A tank was filled with 18 g of oxygen (O2), 75 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 8.5 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x? 3. 13 g of an unknown gas in a tank with a volume of 5.53 L has a pressure of 3.83 atm at 28°C. If the molecular weight of the gas is x g/mol, what is the value of x? 4. Ammonia burns in air as follows:NH3(g) + O2(g) → N2(g) + H2O(g) (unbalanced)If x liters of N2(g) are formed by burning 9.8 L of ammonia and 9.8 L of oxygen with all species at the same temperature and pressure, what is the value of x? 5. Methane (CH4) at 48°C and 776 mmHg has a density x g/L. What is the value of x? 6. A 3.50 L sample of neon has a pressure of 1.03 atm at 17°C. If the sample has…
Question 15 A mixture of gases contains 0.200 mole O2, 0.400 mole N2, and 0.600 mole H2 at 2.00 atm pressure. What is the partial pressure of N2 in the mixture? Group of answer choices 0.667 atm 333 atm insufficient data to answer 1.00 atm
Calcium oxide can be used to "scrub" carbon dioxide from air. CaO(s) + CO2(g) → CaCO3(s) What mass of CO2 could be absorbed by 1.22 g of CaO? answer: 0.957 gWhat volume would this CO2 occupy at STP? L
4. How many hydrogen atoms are there in 25.6 grams of urea, CO (NH2) 2? The molar mass of urea is 60.06 g. 5. Calculate the volume of SO3 gas as much as 16 grams when measured at: a. STP state b. a temperature of 57 ° C and a pressure of 1 atm c. a certain temperature and pressure if the volume of 0.25 moles of N2 gas is 7 liters please help me, I still don't understand
A glass container was initially charged with 2.30 moles of a gas sample at 5.00 atm and 21.7 \deg C. Some of the gas was released as the temperature was increased to 33.1 deg C, so the final pressure in the container was reduced to 1.50 atm. How many moles of the gas sample are present at the end? Only typed solution
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. If an air bag has a volume of 53.4 L and is to be filled with nitrogen gas at a pressure of 1.07 atm and a temperature of 23.7˚C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas. Answer sig figs
QUESTION 6 Calculate the root mean square velocity for the NO2 molecules in a sample of NO2 gas at 11.8°C. (R = 8.3145 J/K mol) 0.392 m/s 7104 m/s 392.9 m/s 471.2 m/s QUESTION 7 The valve between the 3.00-L bulb, in which the gas pressure is 1.20 atm, and the 2.00-L bulb, in which the gas pressure is 3.30 atm, is opened. What is the final pressure in the two bulbs, the temperature remaining constant? 2.46 atm 1.98 atm 0.480 atm 2.04 atm QUESTION 8 A 6.59-g sample of Copper nitrate, Cu(NO3)2, molar mass = 187.56 g/mol, is heated in an evacuated cylinder with a volume of 3.39 L. The salt decomposes when heated, according to the equation: Cu(NO3)2(s) → CuO(s) + NO2(g) + O2(g) Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a…