A student performed the experiment described in this module, using 6.00 mL of a 3% H2O2 solution with a density of 1.03 g mL-1. The water temperature was 22 ° C, and the barometric pressure in the laboratory was 30.30 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 65.40 mL of O2. (10) Calculate the molar volume of O2 at STP.

A student performed the experiment described in this module, using 6.00 mL of a 3% H2O2 solution with a density of 1.03 g mL-1. The water temperature was 22 ° C, and the barometric pressure in the laboratory was 30.30 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 65.40 mL of O2. (10) Calculate the molar volume of O2 at STP.

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

A gaseous solution contains 1.6 g oxygen, 16 g sulfur dioxide. and 5.1 g hydrogen sulfide. What is the mole fraction of hydrogen sulfide?
The answer 6.106*10^3 is incorrect. It is something else, thank you!
Insects do not have lungs as we do, nor do they breathe through their mouths. Instead, they have a system of tiny tubes, called tracheae, through which oxygen diffuses into their bodies. The tracheae begin at the surface of the insect's body and penetrate into the interior. Suppose that a tracheae is 1.34 mm long with a cross-sectional area of 2.46 x 10-9m2. The concentration of oxygen in the air outside the insect is 0.794 kg/m3, and the diffusion constant is 1.26 x 10-5 m2/s. If the mass per second of oxygen is diffusing through a trachea is 1.66 x 10-12 kg/s, then find the oxygen concentration at the interior end of the tube.
80 g of CaCO3 is treated with 0.500 L of a 1.00M solution of HCl. What volume of CO2 gas, measured at 25˚C and 800. mm Hg can be obtained? CaCO3(s) + 2HCl(aq) ® CO2(g) + CaCl2(aq) + H2O(l) Show all equation and all calculations involved to get full marks. Hint: this is a limiting type question Use the following questions as guide and include them in your answer. the limiting reactant is? the maximum number of moles of CO2 gas that can be produced is? the volume of CO2 gas that can be produced from this reaction is?
If the partial pressure of N2 is 2.70 x 105 Pa and the partial pressure of Ne is 5.00 x 105 Pa in a given mixture, what is the mole fraction of Ne (XNe)?
1.If the partial pressure of N2 is 3.10 x 105 Pa and the partial pressure of Ne is 4.75 x 105 Pa in a given mixture, what is the mole fraction of Ne (XNe)? What type(s) of intermolecular forces must be overcome when liquid dipropyl ether (CH3CH2CH2-O-CH2CH2CH3) vaporizes? (You may select more than one. Incorrect answers will be penalised.) Question 2 options: a dipole-dipole forces b dispersion forces c hydrogen bonds d covalent bonds
- Exhaust gas from an automobile contains air and 10^-5 mole fractions of COin air at 25 degC and 1.2 atm. Express this concentration as a mass concentration (kg/m3).
How much carbon dioxide gas (mole percent) is dissolved in a bottle of sparkling water if the manufacturer used a pressure of 2.68 atm in the bottling process at 25°C? HCO2inwater=1630atm and PsatH2O=3.166kPa at 25°C. Assume xH2O=1.
A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the value of KC at 800. K?
In the fermentation of sucrose Calculate how many milliliters of CO2 (at STP) would be produced assuming all of the sucrose were consumed during fermentation. with 10g of sucrose.