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Chemistry
Q:
What is the total pressure in a 10.0 L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0C?
A) 0.306 atm
B) 0.681 atm
C) 0.693 atm
D) 0.998 atm
Q:
A balloon contains 0.76 mol N2, 0.18 mol O2, 0.031 mol He and 0.026 mol H2 at 739 mm Hg. What is the partial pressure of O2?
A) 19 mm Hg
B) 23 mm Hg
C) 130 mm Hg
D) 560 mm Hg
Q:
A 10.0-L flask containing He, 2.00 mole of Ar, and 3.00 mole of Ne has a total pressure of 24.5 atm at 25C. How many moles of He are in the flask?
A) 5.00 mol
B) 10.0 mol
C) 114 mol
D) 119 mol
Q:
At STP how many liters of NH3 can be produced from the reaction of 6.00 L of N2 with 6.00 L of H2?N2(g) + 3 H2(g) -> 2 NH3(g)A) 5.48 LB) 4.30 LC) 1.34 LD) 2.69 L
Q:
How many liters of SO3(g) are produced at 25C and 1.00 atm from the combustion of 1.00 kg of coal which is 1.00% S by weight? Assume all the sulfur in the coal ends up as SO3.
A) 0.640 L
B) 5.08 L
C) 7.63 L
D) 11.4 L
Q:
How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 2.46 atm and 45C in the reaction shown below?XeF6(s) + 3 H2(g) -> Xe(g) + 6 HF(g)A) 3.65 gB) 4.46 gC) 13.4 gD) 40.2 g
Q:
How many liters of oxygen are needed to exactly react with 27.8 g of methane at STP?CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l)A) 19.5 LB) 39.0 LC) 77.6 LD) 85.0 L
Q:
A lungful of air (500 mL) contains 4.1% CO2 by volume. How many grams of KO2(s) is needed to remove the CO2 from a lungful of air at STP according to the following reaction?4 KO2(s) + 2 CO2(g) -> 2 K2CO3(s) + 3 O2(g)A) 0.065 gB) 0.13 gC) 0.26 gD) 1.2 g
Q:
When 15.0 g of zinc metal reacts with excess HCl, how many liters of H2 gas are produced at STP?
A) 0.229 L
B) 0.458 L
C) 5.14 L
D) 10.3 L
Q:
At STP how many grams of Mg are required to produce 35 mL of H2 in the reaction shown below?Mg(s) + 2 HCl(aq) -> H2(g) + MgCl2(aq)A) 0.035 gB) 0.038 gC) 26 gD) 29 g
Q:
The action of some commercial drain cleaners is based on the following reaction:2 NaOH(s) + 2 Al(s) + 6 H2O(l) ->2 NaAl(OH)4(s) + 3 H2(g)What is the volume of H2 gas formed at STP when 4.32 g of Al reacts with excess NaOH?A) 2.39 LB) 3.59 LC) 5.38 LD) 5.87 L
Q:
Chloroform is a volatile liquid once commonly used in the laboratory but now being phased out due to its ozone depletion potential. If the pressure of gaseous chloroform in a flask is 195 mm Hg at 25C and its density is 1.25 g/L, what is the molar mass of chloroform?
A) 10.0 g/mol
B) 76.3 g/mol
C) 119 g/mol
D) none of the above
Q:
Given three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at -20C, cylinder B is at -15F, cylinder C is at 260 K. Which cylinder contains the largest mass of oxygen?
A) cylinder A
B) cylinder B
C) cylinder C
D) All cylinders contain the same mass of O2.
Q:
Which of the following would have a density of 1.21 g/L at 7.0C and 0.987 atm?
A) Ar
B) N2
C) Ne
D) O2
Q:
One mole of which gas has the greatest density at STP?
A) Ar
B) N2
C) CO
D) All three gases have the same density.
Q:
What is the density of fluorine gas at STP?
A) 0.590 g/L
B) 0.848 g/L
C) 1.55 g/L
D) 1.70 g/L
Q:
A 0.286-g sample of gas occupies 125 mL at 60. cm of Hg and 25C. What is the molar mass of the gas?
A) 5.9 g/mol
B) 44 g/mol
C) 59 g/mol
D) 71 g/mol
Q:
Cyanogen is a gas which contains 46.2% C and 53.8% N by mass. At a temperature of 25C and a pressure of 750 mm Hg, 1.50 g of cyanogen occupies 0.714 L. What is the molecular formula of cyanogen?
A) CN
B) C2N2
C) C3N4
D) C4N5
Q:
What is the Celsius temperature of 100.0 g of chlorine gas in a 40.0-L container at 800 mm Hg?
A) -91C
B) 91C
C) 182C
D) 364C
Q:
What is the volume of 10.0 g of argon gas at 157C and 2.50 kPa pressure?
A) 1.29 L
B) 3.53 L
C) 131 L
D) 358 L
Q:
How many grams of O2 gas are there in a 5.00-L cylinder at 4.00 103 mm Hg and 23C?
A) 17.3 g
B) 34.4 g
C) 446 g
D) 2.63 104 g
Q:
A gas occupies 22.4 L at STP and 14.5 L at 100C and 2.00 atm pressure. How many moles of gas did the system gain or lose?
A) 0.06 moles gained
B) 0.03 moles gained
C) 0.03 moles lost
D) 0.05 moles lost
Q:
A steel bottle contains argon gas at STP. What is the final pressure if the temperature is changed to 115C?
A) 0.704 atm
B) 0.768 atm
C) 1.30 atm
D) 1.42 atm
Q:
A 1.00 L flask contains nitrogen gas at 25C and 1.00 atm pressure. What is the final pressure in the flask if an additional of N2 gas is added to the flask and the flask cooled to -55C?
A) 1.28 atm
B) 2.01 atm
C) 2.56 atm
D) 3.29 atm
Q:
A 75.0 L steel tank at 20.0C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many grams of acetylene are in the tank?
A) 4.33 g
B) 6.01 g
C) 113 g
D) 1650 g
Q:
A 1.75 L container filled with CO2 gas at 25C and 225 kPa pressure springs a leak. When the container is re-sealed, the pressure is 185 kPA and the temperature is 10C. How many moles of gas were lost?
A) 0.0213 mol
B) 0.463 mol
C) 0.561 mol
D) 2.16 mol
Q:
How many molecules of N2 are in a 500.0 mL container at 780 mm Hg and 135C?
A) 8.76 1021
B) 9.23 1021
C) 2.65 1022
D) 2.79 1022
Q:
Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains CH4, flask B contains CO2, flask C contains N2. Which flask contains the largest number of molecules?
A) flask A
B) flask B
C) flask C
D) All flasks contain the same number of molecules.
Q:
If the number of moles of gas is doubled at constant temperature and volume, the pressure of the gas
A) is halved.
B) is doubled.
C) is quadrupled.
D) remains the same.
Q:
What is the value of the gas constant, R, in units of ?
A) 1.080 10-4
B) 0.1080
C) 62.36
D) 6.236 104
Q:
A balloon filled with helium gas at 20C occupies 2.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196C, raising the pressure to 5.20 atm. What is the volume of the balloon in the liquid nitrogen?
A) 0.15 L
B) 2.1 L
C) 4.0 L
D) 58 L
Q:
The volume of 350. mL of gas at 25C is decreased to 125 mL at constant pressure. What is the final temperature of the gas?
A) -167C
B) 8.9C
C) 70C
D) 561C
Q:
A gas bottle contains 0.650 mol of gas at 730 mm Hg pressure. If the final pressure is 1.15 atm, how many moles of gas were added to the bottle?
A) 0.0680 mol
B) 0.128 mol
C) 0.717 mol
D) 0.778 mol
Q:
A basketball is inflated to a pressure of 1.50 atm in a 20.0C garage. What is the pressure of the basketball outside where the temperature is -5.00C?
A) 1.37 atm
B) 1.42 atm
C) 1.58 atm
D) 1.64 atm
Q:
An "empty" aerosol can at 25C still contains gas at 1.00 atmosphere pressure. If an "empty" can is thrown into a 475C fire, what is the final pressure in the heated can?
A) 5.26 10-2 atm
B) 0.398 atm
C) 2.51 atm
D) 19.0 atm
Q:
"Equal volumes of different gases at the same temperature and pressure contain the same molar amounts" is another way of stating
A) Avogadro's law.
B) Boyle's law.
C) Charles' law.
D) Graham's law.
Q:
An approximation of absolute zero was made from an extrapolation of
A) P vs. 1/V
B) V vs. T
C) n vs. V
D) V vs. 1/T
Q:
Which law does the equation, = k represent?
A) Avogadro's law
B) Boyle's law
C) Charles' law
D) Graham's law
Q:
When temperature-volume measurements are made on 1.0 mol of gas at 1.0 atm, a plot V versus T results in a
A) hyperbola.
B) parabola.
C) sine curve.
D) straight line.
Q:
When pressure-volume measurements are made on 1.0 mol of gas at constant temperature , a plot V versus P results in a
A) hyperbola.
B) parabola.
C) sine curve.
D) straight line.
Q:
Which of the following equations represents "Boyle's law"?
A) = k
B) = k
C) PV = k
D) V = nk
Q:
Which one of the following is not used to describe the condition of a gas?
A) number of moles
B) polarity
C) temperature
D) volume
Q:
A container filled with gas is connected to an open-end U-tube manometer that is filled with mineral oil. The pressure in the gas container is 773 mm Hg and atmospheric pressure is 754 mm Hg. What will be the difference in the levels of mineral oil in the two arms of the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively?
A) 1.15 mm
B) 15.6 mm
C) 19.0 mm
D) 314 mm
Q:
If the pressure in a gas container that is connected to an open-end U-tube manometer is 106 kPa and the pressure of the atmosphere at the open end of the tube is 742 mm Hg, the level of mercury in the tube will be
A) 53 mm higher in the arm open to the atmosphere.
B) 53 mm higher in the arm connected to the gas cylinder.
C) 636 mm higher in the arm open to the atmosphere.
D) 636 mm higher in the arm connected to the gas cylinder.
Q:
What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 752 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?
A) 666 mm Hg
B) 743 mm Hg
C) 761 mm Hg
D) 838 mm Hg
Q:
In an open end manometer, one end of a U-tube filled with mercury is attached to a gas-filled container and the other end is open to the atmosphere. If the gas pressure in the container is less than atmospheric pressure
A) Hg will be forced out of the open end of the U-tube.
B) the difference between the Hg levels in the two arms will be greater than 76 cm.
C) the Hg level will be higher in the arm connected to the container.
D) the Hg level will be higher in the arm open to the atmosphere.
Q:
Suppose you needed to closely monitor small changes in pressure inside a container using an open end manometer. For the best accuracy, the substance in the manometer should
A) be a solid.
B) be mercury.
C) have a high density.
D) have a low density.
Q:
If mercury (density = 13.6 g/cm3) at a height of 745 mm Hg in a mercury barometer is replaced with water (density = 1.00 g/cm3), under the same conditions the height of water will be
A) 0.180 ft
B) 2.44 ft
C) 33.2 ft
D) 399 ft
Q:
The pressure in the eye of a hurricane is less than atmospheric pressure. Which one of the following pressure readings could not have been taken in the eye of a hurricane?
A) 15 lbs/in2
B) 69 cm Hg
C) 690 mm Hg
D) 9.22 104 Pa
Q:
Automobile tires are typically inflated to about 30 pounds of pressure per square inch. What is the typical air pressure of a tire in kPa? One atm = 14.70 lb/.
A) 2.0 10-3 kPa
B) 2.0 kPa
C) 2.1 102 kPa
D) 2.1 105 kPa
Q:
Which is the smallest quantity of pressure?
A) 1 atm
B) 1 centimeter of Hg
C) 1 mm Hg
D) 1 pascal
Q:
Which of the following is not equivalent to 1 atm pressure?
A) 10 cm Hg
B) 14.7 lb/in2
C) 101 kPa
D) 760 mm Hg
Q:
The SI unit for pressure is the
A) atmosphere.
B) MM Hg.
C) newton.
D) pascal.
Q:
Pressure is defined as
A) force divided by unit area.
B) force times unit area.
C) mass divided by acceleration.
D) mass times acceleration.
Q:
Which of the following instruments directly measures the pressure of a gas?
A) spectrometer
B) manometer
C) polarimeter
D) gas chromatograph
Q:
Carbon dioxide is a gas which causes environmental concern because of the greenhouse effect. What is the approximate percentage (by volume) of CO2 in the atmosphere?
A) less than 0.1%
B) about 1%
C) about 10%
D) more than 20%
Q:
For the reaction, 2 NH3(g) -> (g) + 3 (g), one would expectA) H to be negative and S to be negative.B) H to be negative and S to be positive.C) H to be positive and S to be negative.D) H to be positive and S to be positive.
Q:
At a given temperature and pressure, which of the following would be expected to have the greatest molar entropy?
A) Br2(s)
B) Br2(l)
C) Br2(g)
D) All of these would be expected to have the same molar entropy.
Q:
Which of the following can be interpreted as a measure of randomness?
A) enthalpy
B) entropy
C) free energy
D) temperature
Q:
Which of CH4(g), C2H2(g), and CH3OH(l) provides the most energy per gram upon combustion and which provides the least?CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l) H = -890 kJ2 C2H2(g) + 5 O2(g) -> 4 CO2(g) + 2 H2O(l) H = -2599 kJ2 CH3OH(l) + 3 O2(g) -> 2 CO2(g) + 4 H2O(l) H = -1453 kJA) C2H2 provides the most energy per gram and CH4 the least.B) C2H2 provides the most energy per gram and CH3OH the least.C) CH4 provides the most energy per gram and CH3OH the least.D) CH4 provides the most energy per gram and C2H2 the least.
Q:
The heat of combustion per mole for acetylene, C2H2(g), is -1299.5 kJ/mol. Assuming that the combustion products are CO2(g) and H2O(l), and given that the enthalpy of formation is -393.5 kJ/mol for CO2(g) and -285.8 kJ/mol for H2O(l), find the enthalpy of formation of C2H2(g).A) -846.1 kJ/molB) -620.2 kJ/molC) -226.7 kJ/molD) +226.7 kJ/mol
Q:
Calculate the enthalpy of combustion per mole for C6H12O6. Assume that the combustion products are CO2(g) and H2O(l).A) -5336 kJ/molB) -2816 kJ/molC) -1939 kJ/molD) 580.7 kJ/mol
Q:
Given that H= -311 kJ for the hydrogenation of acetylene, C2H2:H-CC-H(g) + 2 H2(g) -> CH3-CH3(g)and the following bond dissociation energies, estimate a value for the C-to-C triple bond dissociation energy.A) 1050 kJ/molB) 833 kJ/molC) 807 kJ/molD) 397 kJ/mol
Q:
Use the given average bond dissociation energies, D, to estimate H for the following reaction:CCl(g) + (g) ->C(g) + HCl(g)A) -76 kJB) +76 kJC) 334 kJD) -334 kJ
Q:
Use the given average bond dissociation energies, D, to estimate H for the following reaction:CF(g) + (g) ->C(g) + HF(g)A) -94 kJB) +94 kJC) 316 kJD) -316 kJ
Q:
Use the given average bond dissociation energies, D, to estimate H for the following reaction:CBr(g) + (g) ->C(g) + HBr(g)A) -70 kJB) +70 kJC) 340 kJD) -340 kJ
Q:
Use the given average bond dissociation energies, D, to estimate H for the following reaction:CI(g) + (g)->C(g) + HI(g)A) -32 kJB) +32 kJC) 378 kJD) -378 kJ
Q:
Use the given average bond dissociation energies, D, to estimate H for the reaction of methane, CH4(g), with fluorine according to the equation:CH4(g) + 2 F2(g) -> CF4(g) + 2 H2(g)A) -716 kJB) -318 kJC) +318 kJD) +716 kJ
Q:
One method for making ethanol, C2H5OH, involves the gas-phase hydration of ethylene, C2H4:Estimate H for this reaction from the given average bond dissociation energies, D.A) -580 kJB) -35 kJC) +35 kJD) 580 kJ
Q:
For the reaction 2CH4 (g) + 3 Cl2 (g) -> 2 CHCl3 (l) + 3 H2 (g), H = -118.6 kJ.Hf = -134.1 kJ/mol for CHCl3 (l). Find Hf for CH4 (g).A) -193.4 kJ/molB) -74.8 kJ/molC) 74.8 kJ/molD) 193.4 kJ/mol
Q:
Acetylene torches utilize the following reaction:2 C2H2(g) + 5 O2(g) -> 4 CO2(g) + 2 H2O(g)Use the given standard enthalpies of formation to calculate H for this reactionA) 2512.4 kJB) 1256.2 kJC) -1256.2 kJD) -2512.4 kJ
Q:
Ethyl alcohol is produced by the fermentation of glucose, C6H12O6.C6H12O6(s) -> 2 C2H5OH(l) + 2 CO2(g) H = - 69.1 kJGiven that the enthalpy of formation is -277.7 kJ/mol for C2H5OH(l) and -393.5 kJ/mol for CO2(g), find the enthalpy of formation for C6H12O6.A) -1411.5 kJ/molB) -1273.3 kJ/molC) -740.3 kJ/molD) -602.1 kJ/mol
Q:
Use the given standard enthalpies of formation to calculate ΔH for the following reaction3 Fe2O3(s) + CO(g) -> 2 Fe3O4(s) + CO2(g).A) -5213.4 kJB) -577.2 kJC) -47.2 kJD) +47.2 kJ
Q:
Which equation represents the reaction whose H, represents the standard enthalpy of formation of CHCl3(l) at 25C? (i.e., for which is H = Hf of CHCl3)A) CHCl3(l) -> C(s) + H(g) + 3 Cl(g)B) C(s) + H(g) + 3 Cl(g) -> CHCl3(l)C) C(s) + 1/2 H2(g) + 3/2 Cl2(g) -> CHCl3(l)D) 2 C(s) + H2(g) + 3 Cl2(g) -> 2 CHCl3(l)
Q:
The values of Hf for the three states of benzene are approximately -22 kcal/mol, -11 kcal/mol, and Which is the value for solid benzene?A) -22 kcal/molB) -11 kcal/molC) 20 kcal/molD) cannot be determined without additional information
Q:
Which is expected to have the most negative standard enthalpy of formation?
A) H2(g)
B) O2(g)
C) H2O(g)
D) H2O(l)
Q:
For which should the standard heat of formation Hf, be zero at 25C?A) O(g)B) O2(g)C) O3(g)D) all the above
Q:
Find H for C3H8 (g) + 6 H2O (g) -> 3 CO2 (g) + 10 H2given C3H8 (g) + 3 H2O (g) -> 3 CO (g) + 7 H2 (g) H = 499 kJCO (g) + H2O (g) -> CO2 (g) + H2 (g) H = -41 kJA) 376 kJB) 458 kJC) 540 kJD) 622 kJ
Q:
Find ΔH for BaCO3 (s) -> BaO (s)+ CO2 (g)given 2 Ba (s) + O2 (g) -> 2 BaO (s) H = -1107.0 kJBa (s) + CO2 (g) + 1/2 O2 (g) -> BaCO3 (g) H = -822.5 kJA) -1929.5 kJB) -1376.0 kJC) -284.5 kJD) 269.0 kJ
Q:
Coal gasification can be represented by the equation:2 C(s) + 2 H2O(g) -> CH4(g) + CO2(g) H = ?Use the following information to find H for the reaction above.CO(g) + H2(g) -> C(s) + H2O(g) H = -131 kJCO(g) + H2O(g) -> CO2(g) + H2(g) H = -41 kJCO(g) + 3 H2(g) -> CH4(g) + H2O(g) H = -206 kJA) 15 kJB) 116 kJC) -116 kJD) -372 kJ