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.
Do not worry about the significant figures.If the answer do not match due to significant figures then please comment below......
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ...
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water and oxygen (O2). 2H2O2(1)-2H20 (1) + O2(9) How many moles of H, O, are needed to produce 4.50 mol of H, 0? Express your answer with the appropriate units. OLA OP? n(H2O2) = Value Units Submit Request Answer Part B How many grams of H, O, are required to produce 40.9 g of O,? Express your answer with the appropriate units. T! + O2 ? m(H2O2) = Value...
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 29.0 g of a 7.50% hydrogen peroxide solution?
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°; -...
How many grams of hydrogen peroxide (H2O2) are needed to produce 25.0 g of oxygen? 2H2O2 + 2H2O + O2 25.0g 53.1g 5.88 g 106g 26.6g
Delete CHE 120 Pb.9.Liquid hydrogen peroxide, an oxidizing agent used in many rocket fuel mixtures, releases oxygen gas on decomposition: AHon=-196.1 kJ -2H2O(I)O2(g) 2H2O2(l) What mass of H2O2 decomposes if 2510 kJ is released?
(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...
Hydrogen peroxide can decompose to water and oxygen by the following reaction: 2 H2O2(l) → 2 H2O(l) + O2(g) ΔH = –196 kJ Calculate the value of q when 5.00 g of H2O2(l) decomposes at constant pressure.
Hydrogen gas reacts with oxygen to form water. 2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 233 kJkJ of heat.
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) + 1/2 O2(g) 26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(2) + 1/2O2(g) At 20.0 °C, the half-life for the reaction is 3.05 x 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 8.00 days?
The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ: 2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ A) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol of O2 at atmospheric pressure if the volume change is -3.8 L ? B) What is the value of ΔE in kilojoules.