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
Question
Calculations for experimentally determining R
| Trial 1 | Trial 2 | |
| Mass of Mg ribbon (g) | 0.033 | 0.039 |
| Temperature of H2(g) (°C) | 23.5 | 23.7 |
| Volume of H2 collected (mL) | 33.80 | 38.97 |
| Atmospheric pressure (torr) | 758 | 758 |
| Vapor pressure of water (torr) | ||
| Volume of H2 gas in liters (L) | ||
| Temperature of H2 gas in Kelvin (K) | ||
| Moles of H2 gas (mol) | ||
| Pressure of H2 gas in atmospheres (atm) | ||
| Experimental value of R (L·atm/(mol·K)) |
Average value of R (L·atm/(mol·K)):
Percent error (%)Use 0.08206 L·atm/(mol·K) for the theoretical value of R:
The hydrogen generated in this lab was a product of the reaction between magnesium and hydrochloric acid. Which of these reactants is the limiting reactant?: Magnesium or Hydrochloric Acid? Explain reasonsing.
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 9 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
- n electronic vacuum tube was sealed off during manufacture at a pressure of 1.8 x 10-5 mm of Hg and at 27°C. Its volume is 250 mL. How many gas molecules remain in the tube? 2.45 x 1013 molecules 2.40 x 1010 molecules 1.45 x 1014 molecules 14.50 x 1016 moleculesarrow_forwardHi! I am unsure of how to solve this problem. Thank you!arrow_forwardthe atmospheric pressure in inches Hg (inHg) 30.08 Temperature at beginning of measurements (°C) 20.6 Mass added Syringe volume Reading 1 0.0 5.0 Reading 2 0.300 4.5 Reading 3 0.450 4.2 Reading 4 0.650 4.1 Reading 5 0.950 3.6 Reading 6 1.150 3.1 Reading 7 0.200 5.4 Reading 8 0.400 6.7 Reading 9 0.550 7.5 Reading 10 0.700 8.4 Reading 11 0.900 9.3 Temperature at end of measurements (°C) 20.6 PV Measurements and Calculations Volsyringe (mL) VolT (mL) Mass added (kg) Force (kg·m/s2) Psyr (Pa) PT (Pa) PV (Pa·mL) No mass addedReading 1 5.0 0.000 Increasing the pressureReading 2 4.5 0.300 Reading 3 4.2 0.450 Reading 4 4.1 0.650 Reading 5 3.6 0.950 Reading 6 3.1 1.150 Decreasing the pressureReading 7…arrow_forward
- 0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative molecular mass of hydrogen is 2.02 g mol-1 and the gas constant, R, is 8.314 J K−1 mol−1 a) Calculate the number of moles (round to 2 decimal places): b) Calculate the mass of the gas in g (round to 3 significant figures):arrow_forwardIn this experiment, we will be using the gas inside of a small hand-held lighter. Before the trial, the lighter weighed 46.747 g. After the trial the mass of the lebter was 31.104 g. what is the mass in grams of the gas used? Enter a numeric answer only. A Moving to another question will save this response. «< Question 6 of 10 8:39 AM search 耳 a 22 4/13/2022 hp insert prt sc delete 144 %24 4 %23 & L. 8 6. %3D backspace hor R T Y U P F G L enter D pause t sh C alt ctriarrow_forwardAn extended form of the combined gas law can be developed if moles of gas change. In this extended form, only R is constant, so n₁ and n₂ must be included. n₁T₁ T₂ 1 1 22 Based on this gas law, which of the following are correct relationships describing n₁ and n₂? A n ₁ T₁ = ¹₂₁²₂ 1 1 2 (B) E n n 1 2-7 = T T 1 F n P₁"₁=P₂" 2 P₁ P2 == n "₁ ⒸV₁"₁₁=V₂" ₂ V n 1 n 1 == n 2 P₁V₁ P₂V/2 1 1 22 2arrow_forward
- eq req < 1req For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain constant. V=2.30 L at 22.0 °C V = 4.98 L at ? °C PC V = 120. mL at 281 K V = ? mL at 386 K mL V=49.7 mL at 37.0 °C V = ? mL at 357 K a. APR 30 b. C. Submit Answer 2 mL Retry Entire Group Show Hint tv [Review Topics] Ⓒ 9 more group attempts remaining [References] SENSA SPREC ********* Previous Next Save and Exit 3arrow_forwardpe here to search ? * 2 1 According to the kinetic theory of gases, the average kinetic energy of the gas particles in a gas sample is directly proportional to the O number of moles of gas. O volume. O pressure. O molar mass. O temperature. eTextbook and Media Save for Later Attempts: 0 of 2 used Submit Answer W insert N 3 @ 2 W S 13 * # X alt 3 E D $ 101 4 C R O E LL F % 5 V T G 6 B Y 4 & H 7 no U N 4+ * 8 fo M a 144 ( 9 K V fo ▶11 ) O L fn > A4 P - ; alt { ? + [ 1 = ( } 个 ctrl 1 pause prt. backs 1 tarrow_forward11:32 AM Sun Oct 22 Question 21.a of 34 8% 0.5683 g Submit The following reaction can be used to convert carbon dioxide to oxygen gas. 4 KO₂ (s) + 2 CO₂(g) → 2 K₂CO3(s) + 3 O₂(g) What is the mass in grams of oxygen gas that can be produced from 0.371 grams of carbon dioxide?arrow_forward
- 10001 me r 9 е 9.38 Constants Part A Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen iodide are produced from 165 mL of H2 ? H2 (g) +I2(g)→2HI(g) Express your answer with the appropriate units. HÁ VHI Value %3D Submit Previous Answers Reguest Answer X Incorrect; Try Again Provide Feedbackarrow_forwardGive good hand written solutionarrow_forward
arrow_back_ios
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