Question

Please answer #3!

You will be using 25.00 mL of 3.00% by mass solution ({mass H_2O_2/ mass solution}*100) of hydrogen peroxide. Assume the density of this solution is 1.000 g / mL. If all hydrogen peroxide decomposes to water and oxygen according to the reaction 2H_2O_2 (aq) 2H_2O (I) + O_2(g) What is the total volume of the oxygen gas generated if the temperature is 24 degree C and the pressure is 770 Torr (760 Torr = 1 atm) ? (R = 0.08206 L atm / K mol) (At this point you can ignore the effect of water vapir). By convention, the rate of the reaction is positive so that is the reaction of hydrogen peroxide, In this case d means "change in" just like Delta. Suppose you carry out the decomposition reaction using 25.0 mL of a 0.200 M hydrogen peroxide solution and obtain the following results: 8.62 mL of gas is collected in 120 seconds. Assume atmospheric pressure = 760. Torr (1 atm), room temperature = 25 degree C and the vapor pressure of water is 24. Torr. A how many moles of oxygen are produced per second? What is the change in the concentration of H_2O_2 per second (Delta [H_2O_2]/dt)? What is your hypothesis and what specific procedures do you plan to use to investigate your hypothesis? Do not use the example from the previous page.

Answer 1

For the reaction

$aA + bB \rightarrow cC + dD$

Rate of Reaction = -1/a d[A]/dt = -1/b d[B]/dt = 1/c d[C]/dt = 1/d d[D]/dt

The rate of the reaction will be depend upon the stichiometric coefficients of the balanced reaction, this is the reason rate of change of H2O2 is twice the rate of change of O2 in the reaction

Since according to the answer 5.6 * 10^(-6) = 2 * 2.8 * 10^(-6)