Concept explainers
(a)
Interpretation:
The masses of O2 , CO2 , and H2 O transferred to the blood should be calculated.
Concept introduction:
The
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(b)
Interpretation:
The volume of air exhaled per milliliter inhaled should be calculated.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(c)
Interpretation:
The rate this individual losing weight due to breathing should be calculated.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(d)
Interpretation:
The effect of atmospheric pressure on the rate of oxygen transfer in the blood should be explained.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
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Chapter 5 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.arrow_forwardButane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)arrow_forwardAt the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forward
- 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…arrow_forwardAt 100 kPa and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8) combusts, producing 18.0 g CO2 . Calculate the mole fraction of each gas in the initial mixture. Assume complete combustion.arrow_forwardWhen heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s) + CO₂(g) What is the mass of calcium carbonate needed to produce 35.0 L of carbon dioxide at STP? Express your answer with the appropriate units. View Available Hint(s) mass of CaCO3 Submit = Part B 0 370.8 HÅ atm Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining ? Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10 (9) + 1302 (g)→8CO2 (g) + 10H₂O (1) At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 2.20 g of butane? Express your answer with the appropriate units.arrow_forward
- On a summer day, you take a road trip through Death Valley, California, in an antique car. You start out at a temperature of 21°C, but the temperature in Death Valley will reach a peak of 51°C. The tires on your car hold 15.6 L of nitrogen gas at a starting pressure of 249 kPa. The tires will burst when the internal pressure (Pb) reaches 269 kPa. Answer the following questions and show your work. How many moles of nitrogen gas are in each tire? What will the tire pressure be at peak temperature in Death Valley? Will the tires burst in Death Valley? Explain. If you must let nitrogen gas out of the tire before you go, to what pressure must you reduce the tires before you start your trip? (Assume no significant change in tire volume.)arrow_forwardStoichiometry with Partial Pressure Gas jar Gas collects here Trough of water Bee hive shelf Reaction mixture 2 KCIO, 3(s) + > 2 KCI (s), 30 2(g) A sample of KCIO3 is partially decomposed by heating, producing O2 gas that is collected safely over water. The volume of total gas collected is 2.50 x 10-4 m³ at 26 °C, giving 101.99 kPa total pressure. How many grams of KCIO3 were decomposed? What atom was oxidized? What atom was reduced? The pressure of water vapor at 26 °C is 25 torr. SHOW ALL WORK!arrow_forwardAt 1.00 atm and 0 ∘C, a 5.04 L mixture of methane (CH4) and propane (C3H8) was burned, producing 15.7 g CO2. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane= Xpropane=arrow_forward
- + |/ 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 MOSISOarrow_forwardIn which of the following reactions for ideal gas AU = AH 2SO2(g) + 202==> 2SO3(g) .a 2H2(g)+O2(g)===> 2H2O (g) » o H2(g)+Cl2(g)==> 2HCI(g)c O N2(g) + 2H2(g)==> 2NH3(g).darrow_forwardBackground: Many metals react with hydrochloric acid to produce hydrogen gas and metal ions. In this Lab you will use Magnesium: Mg(s) + 2 H+(aq) → H2(g) + Mg2+(aq) The moles of hydrogen gas produced can be determined using the Ideal Gas equation, PV = nRT. Useful Information Pressure of water vapor at 18.8 °C = 16.3 torr P(gases in buret) = P(hydrogen gas) + P(water vapor) PV= nRT where P is in atm, V is in L, and T is in K TK = Tºc + 273 l.0 atm = 760 tor R = 0.082 L atm /K mol Data Volume of water added to the 50 mL buret that has uncalibrated bottom 1.0 mL Buret reading after addition of 1.00 mL water 49.50 mL Mass of metal sample 0.038 g Temperature of water (and thus temperature of gases). 18.8 °C Buret reading of gases 36.9 mL Barometric pressure 760 torr QUESTION What is the partial pressure of water vapor at 18.8 °C? (1…arrow_forward
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