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Concept explainers
(a)
Interpretation:
For the given situations, it is to be determined that whether both liquid and gas are present (L/G), only gas is present (G), or situation is impossible (I).
In flask I, the pressure is 256 mm of Hg.
Concept introduction:
The vapor pressure of a liquid is pressure exerted by its vapor which are present just above its surface.
(b)
Interpretation:
For the given situation, if both liquid and gas are present (L/G), only gas is present (G), and situation is impossible (I) needs to be determined.
In flask II, the pressure is 135 mm of Hg.
Concept introduction:
The vapor pressure of a liquid is pressure exerted by its vapor which are present just above its surface.
(c)
Interpretation:
For the given situation, if both liquid and gas are present (L/G), only gas is present (G), and situation is impossible (I) needs to be determined.
In flask III, the pressure is 165 mm of Hg at 30°C, if temperature is decreased to20°C, the pressure becomes 159 mm Hg.
Concept introduction:
The vapor pressure of a liquid is pressure exerted by its vapor which are present just above its surface.
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Chapter 9 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- A 0.517 g sample of a metal, M, reacts completely with sulfuric acid according to M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 235 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal.arrow_forwardHow would you answer these questions?arrow_forwardAssume 402.46 g of dry ice (solid CO2) is placed in an empty 26.66L closed tank. Determine the pressure in the tank in atmospheres at a temperature of 41.88°C. Assume that all the CO, has been converted into gas. (Molar Mass CO2 = 44.01) K = 273.15 +°C %3D R = 0.08206 (L*atm)/(mol*K) Give your answer to 2 decimal places. 近arrow_forward
- III.) Calculate Vmax and Km · S (mol·1") v, mol·l"-min 4.10 x 10° 1.77 x 10 9.50 x 10* 1.73 x 10* 5.20 x 10* 1.25 x 10* 1.06 x 10* 1.03 x 10* 4.90 x 10 8.00 x 10* 1.06 x 10* 6.70 x 10 5.10 x 10° 4.30 x 10* -6arrow_forwardWhich of the following statements are true? Which are false? Why is each true or false? (e) When steam at 100°C in an autoclave is heated to 120°C, the pressure within the autoclave Increase. (f) When using the ideal gas law for calculations, temperature must be in degrees Celsius.arrow_forward1. Calculate the volume of carbon dioxide adjusted to 25 °C and 1 atm, that plants need to make 1.00 g glucose, CóH12O6, by photosynthesis in the reaction 6CO2(g) + 6H20(I) C6H1206(s) + 602 (g).arrow_forward
- Elemental analysis of an organic liquid with a fishy odour gives the following elemental mass percentages: H 14.94 % C 71.22% N 13.84 %. Vaporization of 270 mg of an impure sample in a 150-mL bulb at 150oC gives a pressure of 435 torr. What is the molecular formula of the compound, and the % purity of the sample?arrow_forwardCould you help explain the first answer in words? I don't know how to explain reaction stoichiometry.arrow_forwardA 0.564 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO,(aq) + H, (g) → A volume of 219 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass: g/mol * TOOLS x10"arrow_forward
- Enter your answer in the provided box. A piece of sodium metal reacts completely with water as follows: 2 Na(s)+2H2O(l)->2NaOH(aq)+H2(g)The hydrogen gas generated is collected over water at 23.0\ deg C. The volume of the gas is 291 mL measured at 0.965 atm. Calculate the number of grams of sodium used in the reaction. (The vapor pressure of water at 23.0\deg C=0.027 atm.)arrow_forwardHydrogen, neon and argon are mixed in a cylinder with total pressure of 1.8 atm.The mole fraction of hydrogen and neon are equally 0.35 , what is the partial pressure of argon ? (atomic mass: Ar=40 , H=1, Ne%320 , R= 0.082057 L.atm / (mol.K) )arrow_forward-Volume of trapped gas = 88.57 mL - moles of O2 = 0.00359- Pressure of trapped gas = 756 mmHg- Partial pressure collected O2 =732.2 mm Hg. - temperature = 298.15 Kd. From these results, calculate an experimental value for the ideal gas constant,R in L atm mol–1 K–1. e. Using 0.0821 as the true value for the gas constant, calculate the % error ofthe experiment to the nearest whole number.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
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