A 1.90 g sample of elemental lithium,Li(s) is reacted with water, yielding lithium hydroxide, LIOH, and hydrogen. 2Li(s) + 2H20(1)→ 2LIOH(aq) + H2(g); The H2(g) is collected over water at 18 °C. What are the partial pressures of the two gases (hydrogen and water vapor) when contained in a 1.00/ container at 22 °C? What is the total pressure?

A 1.90 g sample of elemental lithium,Li(s) is reacted with water, yielding lithium hydroxide, LIOH, and hydrogen. 2Li(s) + 2H20(1)→ 2LIOH(aq) + H2(g); The H2(g) is collected over water at 18 °C. What are the partial pressures of the two gases (hydrogen and water vapor) when contained in a 1.00/ container at 22 °C? What is the total pressure?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Fe(s) + H2SO(aq) → FeS0.(aq) + H2(g) The volume of the balloon was 4.8 x10° L. What mass of Fe was…

A: Equation can be written as: Fe(s)+H2SO4→FeSO4(aq)+H2(g) Molar mass of Fe = 56 g/mol H2 = Molar mass…

Q: A mixture of cyclopropane gas, C3H6, and oxygen, O2, in a 1.00:4.00 mole ratio is used as an…

A: Answer :- 84800 Pa The partial pressure of O2 = 84800 Pa.…

Q: Three gases (8.00 gg of methane, CH4CH4, 18.0 gg of ethane, C2H6C2H6, and an unknown amount of…

A: We know that the gaas law is PV=nRT -----(i) where P is pressure of the system,V is…

Q: Scuba divers who suffer from decompression sickness are treated in hyperbaric chambers using a gas…

A: Answer -

Q: If 56.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and…

Q: 40.0 mL of a 3.79 M solution of H2O2 decomposes according to this reaction: 2 H2O2 (aq) → 2 H20(1) +…

A: The reaction taking place is given as, => 2 H2O2 (aq) ------> 2 H2O (l) + O2 (g) Given :…

Q: A student performs an experiment like the one you saw in Experiment 8. The student determines the…

A: Given, Pressure of oxygen is 0.7811 atm Volume of oxygen is 217 ml = 0.217 L Temperature = 298.15 K…

Q: A 6.75 g sample of potassium chlorate (KClO4) is heated and decomposes into potassium chloride and…

A: Using Dalton's law of partial pressure to fins oxygen's partial pressurePtotal = PO2 + PH2O and…

Q: The gas of a certain volcano had the following composition in mole percent: 60.0% CO2, 28.0% H2,…

A: Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to…

Q: Tochloric acid, the following tion takes place s) + 2 HCI(aq) → ZNCI2(aq) 1) culate the volume of H2…

A: Given, Temperature =30 °c = 303 K Mass of Zn = 65.7 g Moles of Zn = mass/Molar mass =…

Q: A 4.0-liter rigid metal can is filled with nitrogen gas at 45 °C to a pressure of 1.125 atm. The can…

Q: 11. Synthesis gas, which is used in the production of ammonia and methanol, among other uses, is…

A: Since PV = nRT where P = pressure in atm V = volume in L n = moles R = 0.0821 T = temperature…

Q: A 250MI stoppered The pressure of the torr. What would the the flask was transfe

Q: Oxygen gas can be prepared by heating potassium chlorate according to the following equation:…

Q: Suppose that a 26.7-mL volume of HCl solution reactions completely with 55.0 mL of aqueous Na2CO3.…

Q: A gas mixture, that has been formulated to simulate the atmosphere of another planet, contains: 320…

A: The atmosphere of another planet contains 320 mg methane, 175 mg argon and 225 mg nitrogen. The…

Q: 8. For the reaction 2H₂O(1) + 2e → H₂(g) + 2OH(aq), calculate the volume of "dry" hydrogen gas…

Q: For many purposes we can treat butane (C₂H₁0) as an ideal gas at temperatures above its boiling…

Q: For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point…

Q: The temperature of your water was 22.4 degrees Celsius. The volume of hydrogen collected was 35.5…

A: Temperature = T = 22.4 °C V = 35.5 mL P = 28.32 inches Hg What was the mass of the magnesium…

Q: What volume of hydrogen gas (in mL) at 707 mm Hg and 42 °C can be produced when 2.1 g of CaCO3(s)…

A: Given- Pressure=707mmHg = 707/760 = 0.9303 atm (1 atm = 750 mmHg) Temperature=42°C = 42 + 273 = 315…

Q: For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point…

Q: Use the ideal gas equation, PV = nRT, to calculate the pressure in torr of 1.823 moles of oxygen gas…

Q: Consider the reaction: Li2O(aq) + CO2(g) Lİ2CO3(s) ----> What volume of cabon dioxide will react…

A: Given :- Li2O(aq) + CO2(g) ---> Li2CO3(s) Mass of Li2O = 1.00 g Molar mass of Li2O = 29.88…

Q: What volume of hydrogen gas (in mL) at 703 mm Hg and 40 °C can be produced when 2.9 g of MgCO3(s)…

A: According to an ideal gas equation PV= nRT Where P= pressure of the gas, V= volume of the gas, n= no…

Q: What volume of hydrogen gas, in mL, is produced from 0.128 g Mg reacting with an excess of HCI at a…

A: A question based on the mole concept. Using the information about the number of moles of reactant…

Q: When zinc metal is added to hydrochloric acid, the following reaction takes place Zn(s) + 2 HCl(aq)…

A: Given,The reaction:Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g)mass of Zn = 71.9 gThe total vapor pressure…

Q: Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following…

A: An ideal gas is a hypothetical gas that has no intermolecular force and has negligible mass.Here we…

Q: Elemental analysis is performed on an organic liquid with a fishy odor. Vaporization of 275.0 mg of…

A: Given:Mass of compound = 275.0 mg = 275.0 ×10-3 g.Volume of Solution = 110 mL = 110×10-3…

Q: What volume of carbon dioxide gas (in mL) at 835 mm Hg and 37 °C can be produced when 2.4 g of…

Q: A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 g of chlorine…

A: Given : Mass of sulfur tetrafluoride i.e SF4 = 17.3 g Mass of chlorine pentafluoride i.e ClF5 = 17.7…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

A 1.90 g sample of elemental lithium,Li(s) is reacted with water, yielding lithium
hydroxide, LIOH, and hydrogen. 2Li(s) + 2H20(1) 2LIOH(aq) + H2(g); The H2(g) is collected over
water at 18 °C. What are the partial pressures of the two gases (hydrogen and water vapor)
when contained in a 1.00 / container at 22 °C? What is the total pressure?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 0.080-g sample of the boron hydride, B4 H10, is burned in pure oxygen to give B2₂ O3 and H₂O. 2 B4 H10 (s) + 11 O₂(g) → 4 B₂O3 (s) + 10 H₂O(g) Calculate the pressure of the gaseous water in a 6.50-L flask at 45 °C. Pressure = mmHg
When 0.1 mol of HCl gas is placed in a 10 liter box at 25 degree C, the pressure is about the same as that observed when 0.1 mol of NH3 is placed in an identical box at the same temperature. However, when 0.05 mol of HCl and 0.05 mol of NH3 are mixed in a 10 Liter box at 25 degree C, a noticeable lower pressure is observed. Explain this behavior.
The partial pressure of water vapor in saturated air at 34 °C is 5.25×10-2 atm. (a) How many molecules of water are in 1.16 cm3 of saturated air at 34 °C? (b) What volume of saturated air at 34 °C contains 0.563 mol of water?
A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
A sample of H2(g) was collected over water in a volume of 12.0 mL at 18 °C under atmospheric pressure of 770. Torr. Partial pressure of water is P(H2O, 18 °C) = 16 Torr. Find the mol’s of H2(g) in the sample
PV=nRT R=0.0821 atm•L/mol•K °C + 273.15 = K 1 atm = 760 mmHg Many metals produce hydrogen gas when dropped in water. For example: Ca (s) +2 H20 (1) → Ca(OH)2 (aq) + H2(g) How much hydrogen gas (in liters) would be produced from dropping 5.0 grams of Calcium into an excess of water, at 25°C and 755 mmHg?
@
Vessel A (volume 16.6 L) contains 30 g of hydrocarbon, and its pressure at 300 K is 1 atm.What is molecular weight of hydrocarbon ?
Suppose that a 26.5-mL volume of HCl solution reactions completely with 55.0 mL of aqueous Na2CO3. The volume of CO2 formed is 137. mL at 26.°C and 726. mmHg. What is the molarity of the HCl solution?
The gas of a certain volcano had the following composition in mole percent: 60.0% CO2, 28.0% H2, 7.40% HCl, 1.80% HF, 2.70% SO2, and 0.100% H2S. What would be the partial pressure of HF in atmospheres if the total pressure was 285 mmHg? 1atm = 760mmHg