Calculate the work done when 1.51 g of H2O2 decomposes at a temperature of 22.0°C, according to the following reaction:
2H2O2(l) → 2H2O(l) + O2(g)
Express your answer to three significant figure
Calculate the work done when 1.51 g of H2O2 decomposes at a temperature of 22.0°C, according...
Calculate the work done when 5.81 g of Cl2(g) reacts with excess P4(s) at 22.0°C, according the the following equation: P4(s) + 10Cl2(g) → 4PCl5(s) Express your answer to three significant figures.
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°; -...
Please show work I am not getting the correct answers 1. Hydrogen peroxide, H2O2, decomposes spontaneously through the following reaction. 2H2O2(aq) 2H2O(g) + O2(g) The kinetics are second order, and the half‐life is 17.3 min when a 1.75 M solution of H2O2 is made. What is the concentration of the solution after 24.8 min? 2. The decomposition of N2O5 occurs by the following reaction: 2N2O5(g) 4NO2(g) + O2(g) The rate constant is experimentally determined to be 3.4 x 10‐4 s‐1....
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.
Hydrogen peroxide (H2O2) decomposes to produce water and oxygen according to the following reaction: 2 H2O2 (l) -----------> 2 H2O (l) + O2 (g) Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? Group of answer choices 2 molecules of H2O2 -----------------> 2 molecules of H2O + 1 molecule of O2 2 mol of H2O2 ----------------->2 mol of H2O + 1 mol of O2 68.0 g of H2O2 -----------------> 36.0 g of H2O...
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...
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.
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...
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
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.