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18 Nov 2019

A student used 4.972 grams of hydrogen peroxide and roughly 10mL of 1.0 M KI and produced a 71.1 mL volume of gas. The experiment was performed at 27 degrees C. The atmospheric pressure was 761.4 torr.

a) What was the partial pressure (in torr) of water vapor in the 100ml cylinder?

b) What was the partial pressure (in torr) of O2 in the 100ml cylinder?

c) What was the partial pressure (in atm) of O2 in the 100ml cylinder?

d) How many moles of O2 were produced?

e) How many moles of H2O2 were consumed?

f) What mass of H2O2 was consumed?

g) What was the percent by mass of H2O2 in the original solution?

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Reid Wolff
Reid WolffLv2
27 Jul 2019

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Related questions

2. A student performed the experiment described in this module,using 5.00 ml of a 2.50% H2O2 solution with a density of 1.01 gml-1. The water temperature was 24 degrees Celsius, and thebarometric pressure in the laboratory was 30.50 in. Hg. After thestudent immersed the yeast in the peroxide solution, she collected43.70 ml of O2.

(A) convert the barometric pressure to torr.

(B) Obtain the water vapor pressure at the watertemperature.

(C) Calculate the pressure, in torr, exerted by the collected O2at the water temperature.

(D) Convert the water temperature, in Celsius to kelvins.

(E) Calculate the volume, in liters, that the collected O2 wouldoccupy at STP.

(F) Calculate the mass of the H2o2 solution.

(G) Calculate the mass of H2O2 in 5.00 ml of the H2o2solution.

(H) Calculate the number of moles of H2O2 reacting.

(I) Calculate the number of moles of collected O2.

(J) Calculate the molar volume of O2 at STP.

(K) calculate the percent error for the experiment.

A student performed the experiment described in this module. The 5.00-mL mass of the 2.15% percent by mass H2O2 solution used was 5.03 g. The water temperature was 23 C, and the barometric pressure was 31.2 in. Hg. After the student immersed the yeast in the peroxide solution, she observed a 38.60-mL volume change in system volume.

(c) Calculate the pressure, in torr, exerted by the collected O2 at the water temperature.

(d) Covert this pressue, in torr, to atmospheres.

(e) Calculate the volume, in milliliters, of collected O2.

(f) Convert this volume, in milliliters, to liters.

(g) Convert the water temperature, in Celsius, to kelvins.

(h) Calculate the mass of 5.00 mL of the H2O2 solution.

(i) Calculate the mass of H2O2 in 5.00 mL of the solution.

(j) Calculate the number of moles of H202 reacting.

(k) Calculate the number of moles of collected O2.

(l) Determine the proportionality constant, R, in L atm mol-1 K-1.

(m) Calculate the percent error for this determination.

please, please please show all work

Using a 25.00 mL of 3.00% by mass solution ({mass H2O2/masssolution}*100) of hydrogen peroxide. Assume the density of thissolution is 1.000 g/mL. If all of the hydrogen peroxide decomposesto water and oxygen according to the reaction

2 H2O2 (aq) <----> 2 H2O (l) + O2 (g)

What is the total volume of oxygen gas generated if the temperatureis 24 degrees Celsius and the pressure is 770 Torr (760 Torr=1atm)? (R=0.08206 L*atm/K*mol) (At this point you can ignore theeffect of water vapor)

Any assistance would be great, its been awhile since I have had anychemistry and don't know how to approach this. I have an idea ofhow to do it, but I haven't done some of the simple stuff in a longtime like converting moles of H2O2 to moles of O2

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