Concept explainers
5-114 Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate based on the following balanced net ionic equation:
(a) How many moles of wet CO (g), collected at 60.°C and 774 torr total pressure, are produced by the complete reaction of 10.0 g of CaCO3 with excess acid?
(b) What volume does this wet CO2 occupy?
(c) What volume would the CO2 occupy at 774 torr if a desiccant (a chemical drying agent) were added to remove the water? The vapor pressure of water at 60.°C is 149.4 mm Hg.
(a)
Interpretation:
The number of moles of wet
Concept Introduction:
Moles of wet
Answer to Problem 86P
The number of moles of carbon dioxide produced is
Explanation of Solution
The weight of calcium carbonate is
The temperature is
The pressure is
The molecular weight of calcium carbonate is calculated below:
The number of moles in
The balanced chemical equation is below:
From the above equation,
Therefore, the number of moles of carbon dioxide produced is
(b)
Interpretation:
The volume of wet
Concept Introduction:
To determine the volume of wet
The relationship between pressure, volume, and temperature, under two sets of conditions, is given by following equation.
Answer to Problem 86P
The value of carbon dioxide produced is
Explanation of Solution
The weight of calcium carbonate is
The temperature is.
The pressure is
The molecular weight of calcium carbonate is calculated below:
The number of moles in
The balanced chemical equation is below:
From the above equation:
Therefore, the number of moles of carbon dioxide produced is
We know that at STP, 1 mole of any gas occupies
Therefore,
Therefore, the volume of
At STP, the value of
Now, convert the pressure from
We know that,
Therefore, the pressure is calculated below:
Now, convert temperature from
We know that,
Therefore,
The relationship between pressure, volume, and temperature, under two sets of conditions, is given by following equation:
Upon rearranging, we get,
By substituting the values of
Hence the value of carbon dioxide produced is
(c)
Interpretation:
The volume of wet
Concept Introduction:
To determine the volume of wet
The relationship between pressure, volume, and temperature, under two sets of conditions, is given by following equation.
Answer to Problem 86P
Explanation of Solution
The weight of calcium carbonate is
The temperature is
The pressure is
The vapor pressure of water at
The molecular weight of calcium carbonate is calculated below:
The number of moles in
The balanced chemical equation is below:
From the above equation:
Therefore, the number of moles of carbon dioxide produced is
We know that at STP, 1 mole of any gas occupies
Therefore,
Therefore, the volume of
At STP, the value of
The pressure is
Now, convert the pressure from
We know that,
Therefore, the pressure is calculated below,
The vapor pressure of water at
Therefore, the pressure is calculated below,
Now, convert temperature from°C to K.
We know that,
Therefore,
The relationship between pressure, volume, and temperature, under two sets of conditions, is given by following equation,
Upon rearranging, we get,
By substituting the values of
Hence the value of carbon dioxide produced is
Want to see more full solutions like this?
Chapter 5 Solutions
Introduction To General, Organic, And Biochemistry
- What mass of KO2 is required to remove 90.0% of the CO2 from a sample of 1.00 L of exhaled air (37°C, 1.00 atm) containing 5.00 mole percent CO2?arrow_forward6-78 (Chemical Connections 6A) Oxides of nitrogen (NO, NO2,N2O3) are also responsible for acid rain. Which acids can be formed from these nitrogen oxides?arrow_forwardHow does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?arrow_forward
- What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?arrow_forwardHow many liters of HCI gas, measured at 30.0 C and 745 torr, are required to prepare 1.25 L of a 3.20-M solution of hydrochloric acid?arrow_forwardGiven that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forward
- (a) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas? °Carrow_forwardSulfur dioxide reacts with oxygen in the presence of plati- num to give sulfur trioxide: 2 SO2(g) + O2(g) → 2 SO3(g) Suppose that at one stage in the reaction, 26.0 mol SO2, 83.0 mol O2, and 17.0 mol SO3 are present in the reaction vessel at a total pressure of 0.950 atm. Calculate the mole fraction of SO3 and its partial pressure.arrow_forwardCalculate the partial pressure of O2 produced from 1.80 L of 0.576 M N2O5 solution at 45 ∘C over a period of 20.8 h if the gas is collected in a 10.3-Lcontainer. (Assume that the products do not dissolve in chloroform.)arrow_forward
- If 14.5g of calcium carbonate decomposes via the following reaction, how many liters of carbon dioxide at a temperature of 303K and 1.02atm will be produced? CaCO3(s)−→−heatCaO(s)+CO2(g) Use R=0.08206L atmmol K for the ideal gas constant. Your answer should have three significant figures.arrow_forward5. Calculate the volume of oxygen consumed at SATP (25 °C, 100kPa) by the combustion of 10.4 kg of propane, C3H8. (arrow_forwardWhile ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 200.mL flask with 1.2atm of ethylene gas and 1.3atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.25atm of ethylene gas and 0.35atm of water vapor. The engineer then adds another 0.30atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax