![EBK GENERAL, ORGANIC, AND BIOLOGICAL CH](https://www.bartleby.com/isbn_cover_images/8220101460288/8220101460288_largeCoverImage.jpg)
EBK GENERAL, ORGANIC, AND BIOLOGICAL CH
3rd Edition
ISBN: 8220101460288
Author: Deal
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Question
Chapter 7, Problem 7.22PP
Summary Introduction
To determine:
The new volume of the bubble outside the volcano.
Introduction:
The ideal gas equation is the combination of Boyle’s law, Charles’s law and the
The ideal gas equation shows the relationship between the pressure, volume, number of moles of gas, gas constant (R) and temperature of the gas.
Expert Solution & Answer
![Check Mark](/static/check-mark.png)
Want to see the full answer?
Check out a sample textbook solution![Blurred answer](/static/blurred-answer.jpg)
Students have asked these similar questions
A student experimentally determines the gas law constant, R, by reacting a small piece of
magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water
in a eudiometer. Based on experimentally collected data, the student calculates R to equal
L'atm
0.0832
mol·K
L'atm
Ideal gas law constant from literature: 0.08206
mol·K
(a) Determine the percent error for the student's R-value.
Percent error =|1.389
(b) For the statements below, identify the possible source(s) of error for this student's trial.
The student uses the barometric pressure for the lab to calculate R.
The student does not equilibrate the water levels within the eudiometer and the
beaker at the end of the reaction. The water level in the eudiometer is 1-inch
above the water level in the beaker.
The student does not clean the zinc metal with sand paper.
The student notices a large air bubble in the eudiometer after collecting the
hydrogen gas, but does not dislodge it.
The universal gas constant, R, is defined as the following:
kg · m²
s2 · K• mol
R = 8.314
What would be its value in the following unit?
lb· cm?
day2 · K• mol
1. Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant?
2. Why does the density of water change with its temperature?
3. If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation?
4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?
Chapter 7 Solutions
EBK GENERAL, ORGANIC, AND BIOLOGICAL CH
Ch. 7 - Prob. 7.1PPCh. 7 - Prob. 7.2PPCh. 7 - Prob. 7.3PPCh. 7 - Given that only polar molecules can participate as...Ch. 7 - Prob. 7.5PPCh. 7 - Prob. 7.6PPCh. 7 - An ion-dipole attraction often occurs when ionic...Ch. 7 - Prob. 7.8PPCh. 7 - Prob. 7.9PPCh. 7 - Prob. 7.10PP
Ch. 7 - Prob. 7.11PPCh. 7 - Prob. 7.12PPCh. 7 - Prob. 7.13PPCh. 7 - Prob. 7.14PPCh. 7 - Prob. 7.15PPCh. 7 - Prob. 7.16PPCh. 7 - Prob. 7.17PPCh. 7 - Prob. 7.18PPCh. 7 - Nitrous oxide, N2O, or laughing gas, is a common...Ch. 7 - An Ambu bag is used in emergency resuscitation....Ch. 7 - Prob. 7.21PPCh. 7 - Prob. 7.22PPCh. 7 - Prob. 7.23PPCh. 7 - As a cylinder of compressed gas empties, the...Ch. 7 - Prob. 7.25PPCh. 7 - Prob. 7.26PPCh. 7 - Prob. 7.27PPCh. 7 - Prob. 7.28PPCh. 7 - Prob. 7.29PPCh. 7 - Prob. 7.30PPCh. 7 - Prob. 7.31PPCh. 7 - Prob. 7.32PPCh. 7 - Prob. 7.33PPCh. 7 - Prob. 7.34PPCh. 7 - Prob. 7.35PPCh. 7 - What component molecules make up a triglyceride?Ch. 7 - Prob. 7.37PPCh. 7 - Prob. 7.38PPCh. 7 - Prob. 7.39PPCh. 7 - Prob. 7.40PPCh. 7 - Prob. 7.41PPCh. 7 - Prob. 7.42PPCh. 7 - Prob. 7.43APCh. 7 - Prob. 7.44APCh. 7 - Prob. 7.45APCh. 7 - Prob. 7.46APCh. 7 - Prob. 7.47APCh. 7 - Prob. 7.48APCh. 7 - Prob. 7.49APCh. 7 - Prob. 7.50APCh. 7 - Prob. 7.51APCh. 7 - Prob. 7.52APCh. 7 - Prob. 7.53APCh. 7 - Prob. 7.54APCh. 7 - A beach ball is filled with 10.0 L of air in a...Ch. 7 - Prob. 7.56APCh. 7 - Prob. 7.57APCh. 7 - Liquid nitrogen is an extremely cold liquid (196...Ch. 7 - A full cylinder of compressed gas is moved to a...Ch. 7 - Prob. 7.60APCh. 7 - Your friend breathes in 1.5 L of helium from a...Ch. 7 - Prob. 7.62APCh. 7 - Prob. 7.63APCh. 7 - Prob. 7.64APCh. 7 - Predict which member of each of the following...Ch. 7 - Predict which member of each of the following...Ch. 7 - A stain on your shirt will not come out when you...Ch. 7 - Prob. 7.68APCh. 7 - Prob. 7.69APCh. 7 - Prob. 7.70APCh. 7 - Prob. 7.71APCh. 7 - Prob. 7.72APCh. 7 - Prob. 7.73APCh. 7 - Prob. 7.74APCh. 7 - Prob. 7.75APCh. 7 - Prob. 7.76APCh. 7 - Prob. 7.77APCh. 7 - Prob. 7.78APCh. 7 - Prob. 7.79APCh. 7 - Soap, phospholipids, and cholesterol are all...Ch. 7 - Describe other components present in a cell...Ch. 7 - Prob. 7.82APCh. 7 - Prob. 7.83CPCh. 7 - Desflurane and sevoflurane are common inhalation...Ch. 7 - Prob. 7.85CPCh. 7 - Prob. 7.86CPCh. 7 - Prob. 7.87CPCh. 7 - Getem Clean, Inc. has hired you as chief chcmnt...Ch. 7 - Prob. 7.89CPCh. 7 - Prob. 1IA.1QCh. 7 - Prob. 1IA.2QCh. 7 - Prob. 1IA.3QCh. 7 - Prob. 1IA.4QCh. 7 - Prob. 1IA.5QCh. 7 - Prob. 1IA.6QCh. 7 - Prob. 1IA.7QCh. 7 - Prob. 2IA.1QCh. 7 - Prob. 2IA.2QCh. 7 - Prob. 2IA.3QCh. 7 - Prob. 2IA.4QCh. 7 - Prob. 2IA.5QCh. 7 - Prob. 2IA.6QCh. 7 - Prob. 2IA.7QCh. 7 - Devise a rule to predict the solubility of an...Ch. 7 - Prob. 1ICCh. 7 - Prob. 2ICCh. 7 - Prob. 3IC
Knowledge Booster
Similar questions
- A metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and temperature of the cylinder when it was initially filled were 120 atm and 75 ◦C, respectively. The molar mass of carbon is 12 g·mol−1 and the molar mass of hydrogen is 1 g·mol−1. a) How many moles of propane are in the cylinder? b) What is the mass of the propane inside the cylinder? c) After some time, the cylinder and its contents cool to 25 ◦C. What is the pressure in the cylinder after it has cooled?arrow_forwardThe vapor pressure of mercury at 20 oC is 1.7 x 10-6 atm. Your lab partner breaks a mercury thermometer and spills most of the mercury onto the floor. The dimensions of the laboratory are 16.0 m x 8.0 m x 3.0 m (l x w x h). At 20 oC, calculate the mass (in grams) of the mercury vapor in the room. Determine if the concentration of mercury vapor exceeds air quality regulations of 5.0 x 10-2 mg/m3. How would you clean up this spell?arrow_forwardA gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 25.3 °C. What was the pressure in the gas tank then?arrow_forward
- When solid calcium carbonate is reacted with aqueous hydrochloric acid, the products of the reaction include aqueous calcium chloride, liquid water, and gaseous carbon dioxide. Calculate the volume of CO₂ gas (in L) collected over water at 25.0 °C when 25.1 g of calcium carbonate is added to excess hydrochloric acid if the total pressure is 911 mm Hg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg.arrow_forwardUse vapor pressure. A student leaving campus for spring break wants to make sure the air in his dorm room has a high water vapor pressure so that his plants are comfortable. The dorm room measures 3.41 mx 4.41 m x 3.90 m and the student places a pan containing 0.874 L of water in the room. Assume that the room is airtight, that there is no water vapor in the air when he closes the door, and that the temperature remains a constant 22 °C. The vapor pressure of water at 22 °C is 19.8 mm Hg. (a) Calculate the pressure that the water vapor would exert if all of the liquid water evaporated. mm Hg (b) Will all of the water in the pan evaporate? [arrow_forwardOxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KCIO3(s)→→→→2KCI(s) + 30₂(g) The product gas, O₂, is collected over water at a temperature of 25 °C and a pressure of 744 mm Hg. If the wet O₂ gas formed occupies a volume of 6.86 L, the number of grams of O₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C. Submit Answer 5 question attempts remainingarrow_forward
- Ideal Gas Law A sample of liquid acetone is placed in a .035 L flask and vaporized by heating to 75°C at 102 atm. The vapor weighs 5.87 g Calculate the number of moles of the acetone. where V = volume in liters P = pressure in atmosphere n = moles T=temperature in Kelvin R= universal gas constant, =0.0821 L atm/mol. K =8.314 L kPa/mol, Karrow_forwardWhen zinc metal is added to hydrochloric acid, the following reaction takes place Zn(s) + 2 HCI(aq) → ZnCl2(aq) + H2(g) Calculate the volume of H2 gas collected over water at 30.0 °C when 65.7 g of zinc is added to excess hydrochloric acid if the total pressure is 695 torr. The vapor pressure of water at 30.0 °C is 31.8 torr.arrow_forward8. For the reaction 2H₂O(1) + 2e¯ → H₂(g) + 2OH(aq), calculate the volume of "dry" hydrogen gas created at a pressure of 745 mm Hg and 25.0 °C when 0.6696 g H₂O are used. The vapor pressure of water at this temperature is 23.8 mmHg. A) 0.479 L B) 0.464 L C) 0.450 L D) 4.18 L E) 4.05 Larrow_forward
- A helium balloon is filled to a volume of 5.60 L at 25 °C. What will the volume of the balloon become if it is put into liquid nitrogen to lower the temperature of the helium to 77 K?arrow_forwardPart A. Multiple Choice Identify the choice that best completes the statement or answers the question. L·atm R = 0.08206 mol · K 1. At 0.982 atm, the height of mercury in a barometer is 0.746 m. If the mercury were replaced with ethanol, what height of ethanol (in meters) would be supported at this pressure? The densities of Hg and ethanol are 13.5 g/cm³ and 0.789 g/cm³, respectively. а. 0.0436 m b. 0.946 m с. 0.760 m d. 12.8 m е. 13.0 marrow_forwardWhen zinc metal is added to hydrochloric acid, the following reaction takes place Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g) Calculate the volume of H₂ gas collected over water at 30.0 °C when 71.9 g of zinc is added to excess hydrochloric acid if the total pressure is 695 torr. The vapor pressure of water at 30.0 °C is 31.8 torr.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning