The following reaction was performed over water: 2H2O2 (l) -> 2H2O (l) + O2 (g) What volume of "dry O2" was obtained if the amount of H2O2 used was 15.0g at a total pressure of 755.5 mmHg at a temperature of 25°C? The vapor pressure of water is 23.8 mmHg at 25°C.
The following reaction was performed over water: 2H2O2 (l) -> 2H2O (l) + O2 (g) What...
The reaction 2H2O2(aq)→2H2O(l)+O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s−1 at 20.0 ∘C. A reaction vessel initially contains 150.0 mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11 g/mL). The gaseous oxygen is collected over water at 20.0 ∘C as it forms. What volume of O2 will form in 73.9 seconds at a barometric pressure of 719.5 mmHg . (The vapor pressure of water at this...
Hydrogen peroxide decomposes into water and oxygen according to the following reaction: 2H2O2(1)→ 2H2O(g) + O2(g) 0.11 g of H2O2 is decomposed in a flask with a volume of 2.50 L. What is the pressure of O2 at 298 K? a. 0.032 atm b. 0.048 atm C. 0.016 atm d. 0.16 atm e. None of the above Predict the signs of AH° and ASº for the following reaction: O2(g) + O2(1) a. + AH°; + AS° b. + AH°; -...
(Part A) Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated by light, heat, or a catalyst. The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from 26.8 g of a 7.50% hydrogen peroxide solution? (Part B) What volume of bromine (Br2) vapor measured at 100.°C and 700. mmHg pressure would...
the following first order reaction has a half life of 22.5
minutes.
2H2O2(aq)
2H2O(l) + O2(g)
a. calculate the rate constant for this reaction.
b. if the initial concentraition of H2O2 is 0.30M, calculate the
amout of H2O2 that reamains after 45 min.
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ Part B: How many kilojoules are released when 3.05 moles of H2O2 reacts? Express your answer with the appropriate units. Part C: How many kilojoules are released when 277 g of O2 is produced? Express your answer with the appropriate units.
Question 5 What is AHºp for the following reaction? 2H2O2(1) - 2H2O(1) + O2(g) AH® (H2O(l) = -285.8 kJ/mol, AHºf(H2O2(0) = -187.6 kJ/mol -98.2 kJ/mol @ -473.4 kJ/mol -196.4 kJ/mol 98.2 kJ/mol -946.8 kJ/mol Previous
Consider the reaction: 2H2O2(l)2H2O(l) + O2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.40 moles of H2O2(l) react at standard conditions. S°surroundings = J/K
For the reaction 2H2O2(l)2H2O(l) + O2(g) H° = -196.0 kJ and S° = 125.7 J/K The equilibrium constant for this reaction at 305.0 K is . Assume that H° and S° are independent of temperature. AND The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K. NH4I(s) NH3(g) + HI(g) If ΔH° for this reaction is 182 kJ, what is the value of Kp at 775 K? Kp =
The reaction 2H2O2(aq)->2H2O(l)+O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s^-1 at 20.0 degrees Celsius. A reactionvessel initially contains 150.0mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11g/mL). The gaseous oxygen is collected over water at 20.0 degreesCelsius as it forms.)The vapor pressure of water at this temperature is 17.5mmHg )
2H2O2(l)2H2O(l) + O2(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.37 moles of H2O2(l) react at standard conditions.