Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
Transcribed Image Text:| 2. A 0.500 g impure sample of LINO; is heated, causing it to decompose according to the
following equation:
4LINO:(s) 2Li,0(s) + 4NO:(g) + O:(g)
The gases produced are collected over water at 27°C and 1.00 atm external pressure, and
occupy a volume of 55.2 mL. Calculate the partial pressure of O, in the mixture? What is the
percentage of LINO; in the sample? The partial pressure of water is 26.7 mm Hg at 27°C.
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
Trending nowThis is a popular solution!
Step by stepSolved in 3 steps
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
- 14.1 L of CO2 at 61.47 °C occupies a volume of 23.3 L when the temperature is changed. What is the new temperature (K)? Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Convert temperature(s) to K, and enter with proper s.f. If the term doesn't apply in this problem enter 0. Enter a question mark for the variable being calculated. Do not leave any blank empty. P1 = V1 = T1= n1= P2= V2= T2= n2= Rearrange the gas law equation needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressures = P1, P2; volumes = V1, V2; temperatures = T1, T2, moles = n1, n2 Terms in the numerator: , Terms in the…arrow_forward||| O STATES OF MATTER Calculating the mass of a gas collected over water Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. Suppose the CO gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 63.9 mL. x10 X collected Ś gas water 0/5 Sketch of a gas-collection apparatus Calculate the mass of CO that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases. 1 g 1 chemical reaction SIarrow_forward+7 (A) 15.2 L B) 0 C) +3 D) -2 19. 68.1 g solid CaCO3 is mixed with excess HC1. What is the volume of CO2 will be collected at 0.0 °C, and 1 atm. (Molar mass CaCO3 = 100.08 g/mol, CO₂ = 44.1 g/mol CaCO3 (s) + 2 HCl(aq) → H₂O (1) +CaCl2 (aq) + CO₂(g) C) OL B) 29.9 L C D) 155 L 20. A gas sample has an initial volume of 0.500 L and initial pressure of 1.0 atm. Wha the volume when the pressure of the sample is decreased to 0.50 atm? Assume the temperature and number of moles of the gas are constant. P₁V₁ = P₂1 A) .0 L B) 0.025 Larrow_forward
- Please don't provide handwritten solution ...arrow_forwardThe catalytic decomposition of hydrogen peroxide yields oxygen gas and water, according to the reaction given below. In an experiment, the decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 0.976 atm. (Pwater = 0.032 atm at 25°C) 2 H2O2(aq) → 2 H2O(l) + O2(g) If the original H2O2 solution had a volume on 500 mL, what was the molar concentration of hydrogen peroxide prior to decomposition?arrow_forward10 mol of NH3 (g) were placed in a previously evacuated 20-L container. After a sudden temperature rise to 961.4 K, 80% of ammonia dissociated into hydrogen and nitrogen according to the reaction: 2/3 NH3 (g) --> 1/3 N2 (g) + H2 (g) What is the total pressure of the mixture if all gases are ideal? (Answer in sig figs)arrow_forward
- d. The gas is NO2 and the molar mass is 46 g-mol-'. What is the percent yield when 1.72 g of H2O2 decomposes and produces 375 mL of O2 gas measured at 42 °C and 1.52 atm? The molar mass of H2O2 is 34.02 g-mol-1. 2H2O2(aq) → 2H20(1) + O2(g) Data sheet and Periodic Table Select one: O a. 15.3% O b. 30.7% O c 43.7% O d. 87.2% What is the total volume of gases produced when 3.0 L of nitrogen trichloride (NCI3) decomposes into chlorine and nitrogen at a c and temperature? 2NCI3(g)→N2(g) + 3CI2(g)arrow_forward11. What volume of hydrogen gas at STP may be prepared by the reaction of 4.54 g of gallium with 110. mL of 1.75M hydrochloric acid? The unbalanced equation is shown below. (Assume STP is 0 °C and 1 atm) Ga (s) + HCI (aq) GaClз (aq) + H2 (g)arrow_forwardA catalytic converter in an automobile uses a palladium or platinum catalyst to convert carbon monoxide gas to carbon dioxide according to the following reaction: 2C0(g) + 02(9) → 2CO2(g) Part A A chemist researching the effectiveness of a new catalyst combines a 2.0: 1.0 mole ratio mixture of carbon monoxide and oxygen gas (respectively) over the catalyst in a 2.45- L flask at a total pressure of 735 torr and a temperature of 552 C. When the reaction is complete, the pressure in the flask has dropped to 554 torr. What percentage of the carbon monoxide was converted to carbon dioxide?arrow_forward
- Three gases (CO, 02, and N) are trapped in individual bulbs of difterent volumes below. When the valves are opened, the individual gases expand and occupy the entire volume (10.00 L) of the apparatus. Assume that the temperature is constant. The mole fraction of each gas is equal to the partial pressure of a gas divided by the total pressure %3D What is the mole fraction of N2(g) in the mixture? (XN2 = PN2/Ptotal) Bulb Gas Volume (1) Pressure (atm) Carbon dioxide 3.00 1.00 Oxygen 1.00 1.00 Nitrogen 6.00 3.00 III O a 0.81 O b. 2.23 O 1.80 d. 0.500 0.654 f. The temperature must be knownarrow_forwardSodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0°C and 1.00 atm How much CO_2 (in liters) is produced by the reaction of 6.00 kg of sodium bicarbonate with excess hydrochloric acid? Hint: one step uses the mole ratio. NaHCO_3(s) + HCI_(aq) -----> NaCI + H₂O_(l) + CO_2(g)arrow_forwardA tank contains 2 m³ of a gas which is 70% methane, 25% ethane, and 5% nitrogen by volume. The mixture is at 20 °C and 25.66 atm, the average molar mass of the gas is 20.1 kg/kmol (R=0.082 m³.atm/kmol.K) Component CH4 C2H6 N2 2.27 kmol Using Kay's method, what is the number of moles of this mixture in the tank? 4.27 kmol 6.27 kmol Tc, K Pc, atm 190.6 45.4 305.4 48.2 126.2 33.5 8.27 kmol 00 0.008 0.098 0.040arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY