2. Analyze the relationship between percent hydrogen peroxide and volume of gas produced by following the steps below. The graph shows the data collected for various samples with different Rercents, of hydrogen peroxide at 1.00 atm and 298 K. a. What is the percent hydrogen peroxide listed on the bottle? This is the theoretical percent| Theoretical percent: 3% b. On the graph below, locate the value of the volume in ml of O2 that you collected in your experiment. Trace this value from the y-axis to the plotted line and then from the plotted line down to the x-axis to find the percent hydrogen peroxide that corresponds to this volume of O2. Record value with one estimated decimal place. This is the experimental percent. Experimental percent: vo (mL) vs % H,O2 100.0 90.0 80.0 70.0 60.0 50.0 40.0 30.0 20.0 10.0 0.0 1 2 5 % hydrogen peroxide c. Calculate the percent error in your experiment by comparing the theoretical and experimental percents, using the equation below. experimental-theoretical % error = theoretical (ju)O A

2. Analyze the relationship between percent hydrogen peroxide and volume of gas produced by following the steps below. The graph shows the data collected for various samples with different Rercents, of hydrogen peroxide at 1.00 atm and 298 K. a. What is the percent hydrogen peroxide listed on the bottle? This is the theoretical percent| Theoretical percent: 3% b. On the graph below, locate the value of the volume in ml of O2 that you collected in your experiment. Trace this value from the y-axis to the plotted line and then from the plotted line down to the x-axis to find the percent hydrogen peroxide that corresponds to this volume of O2. Record value with one estimated decimal place. This is the experimental percent. Experimental percent: vo (mL) vs % H,O2 100.0 90.0 80.0 70.0 60.0 50.0 40.0 30.0 20.0 10.0 0.0 1 2 5 % hydrogen peroxide c. Calculate the percent error in your experiment by comparing the theoretical and experimental percents, using the equation below. experimental-theoretical % error = theoretical (ju)O A

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

Similar questions

How do you solve the chem question in the picture? A. 22mol B. 20mol C. 12 mil D. 16mol
The molar composition of a gas is 10% H2, 10% O2, 30% CO2 and balance H2O. If 50% H20 condenses, the final mole percent of H2 in a. 10% b. 5% c. 18.18% d. 20 %
Chemistry 151 Week 9- Introduction to Gases POST-LABORATORY QUESTIONS: To solve each of the problems below, first determine the equation you will need from the Introduction section of this lab. (o od wneh n bae Inorl bba of nodemi to mollod os barhU 2 Tonisino adi ot anged lw.cooto o 2. A certain gas held at a temperature of 31.2 °C holds a volume of 458 mL. If the temperature is changed to 55.0 °C, what will be the volume of the gas? i to bi va b d sl a oti l h of do ne ntyiod ba 0gol oni guinm nigomomi d smulow steluls i (ma) ouloV 000 028
16. What is the most nearly the combined volume of 1.0g of hydrogen gas and 7.0g of helium gas when confined at 35°C and 8atm? a. 12.7251Li b. 13.0432Li c. 12.5200Li d. 12.6430Li show complete solution
Pls do fast and i will give like for sure Try to give solution in typed form
3. A mixture of Na2CO3 and NaHCO3 has a mass of 22.0 g. Treatment with excess HCI solution liberates 6.00 L CO2 at 25°C and 0.947 atm pressure. Determine the percent Na2CO3 in the mixture. Hint: Remember, percent mass is the ratio of the mass of substance and the total mass. 55% O 35% 40% 65%
The LEL of n-hexane is 2.5% If a combustible gas meter reads 10% LEL, what is the vapor concentration, IN PPM, in the tested atmosphere a. 025 b. 25,000 2500 d. 10,000
Answer the following with neat solutions. Will upvote who will answer it all and completely.
Consider the reaction: 4 PH3 (g) → P4 (g) + 6 H2 (g) In the reaction above, 0.075 mole of H2 is produced in a 2.0-L container over some time period. What concentration of PH3 is consumed over the same time period?
Please answer
A 1.35 mol gas sample occupies a volume of 345 mL. How many additional moles of the gas must be added to obtain a volume of 456 mL at constant pressure and temperature. O 1.78 mol O 1.02 mol O 1.87 mol O 0.330 mol O 0.430 mol Next
Directions: Solve for what is being asked in each problem. Show your solutions and box your final answer. 1. If oxygen exerts a 4atm of pressure in a mixture and the total pressure of the system is 10 atm, what would be the mole fraction of oxygen in the mixture? 2. Compute for the mole fraction of neon exerting a pressure of 0.28 atm in a gas mixture which has a total pressure of 1.15 atm.