A 6.00 mL solution of hydrogen peroxide decomposes generating 20.4 mL of oxygen gas at 1.10 atm and 20.0 oC.  Calculate the percent mass by volume of hydrogen peroxide solution given the following equation. 2H2O2 ⟶ 2H2O + O2 Group of answer choices 0.265 % 0.0915% 0.530% 1.06% 31.1%

Q: If 78.1 g of solid CaCO3 and 480 mL of 0.458 M aqueous H2SO4 are reacted stoichiometrically…

A: Determine number of moles of each reactant: 1 mL = 0.001 L From the balanced equation, it is clear…

Q: The Oxygen Room  A room with dimensions 7.00m×8.00m×2.50m7.00m×8.00m×2.50m is to be filled with…

A: Given, Temperature = 22.0°C = 22.0+273 =295K   Pressure = 1.0 atm  Volume of oxygen is equal to the…

Q: Air contains nitrogen, oxygen, argon, and trace gases. If the partial pressure of nitrogen is 592 mm…

A: Given: Partial pressure of Nitrogen = 592 mm Hg Partial pressure of Oxygen = 160 mm Hg Partial…

Q: Calculating partial pressure in a gas mixture 0/5 A 8.00 L tank at 24.9 °C is filled with 9.56 g of…

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Q: What volume of oxygen gas at STP is required to react with 10 g of potassium metal according to the…

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Q: What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's…

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Q: What is the volume in liters of hydrogen gas that would be produced by the reaction of 59.0 g of Al…

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Q: When exposed to UV light, chlorine and hydrogen gases explosively combine to form hydrogen chloride…

A: Given information:Pressure of each chlorine and hydrogen atom = 7.0 atmTemperature and volume are…

Q: P4O10 was created by reacting with a phosphorus solid with 0.360 kg of O2 under standard temperature…

A: Ideal gas equation is: PV = nRT                                                           . . . (1)…

Q: What volume of ammonia gas, measured at 782.0 mmHg and 38.6oC, is needed to make 1.28 g of ammonium…

A: The ideal gas equation is as follows,                                 P V = n R T Where P is the…

Q: Composition of Dry Air at Sea Level Gas Mole% N2 78.084 O2 20.946 Ar   0.934 CO2   0.0345 Ne…

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Q: What volume of gas, in liters at 305 K and 1.10 atm, is formed from the reaction of 50.0 grams of…

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Q: Aqueous sulfurous acid (H2SO3) was made by dissolving 0.200 L of sulfur dioxide gas at19°C and 745…

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Q: What volume of carbon dioxide gas is produced at STP by the decomposition of 0.150 g CaCO3 via the…

A: The decomposition of CaCO3 takes place as follows: Chemical equation: CaCO3(s)    →  CaO(s )   +…

Q: Phosphorus trifluoride is a highly toxic gas that reactsslowly with water to give a mixture of…

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Q: gas mixture of 2.31 g NH3, 31.2 g N2, and 0.58 g mol of H2O vapor is contained at a total pressure…

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Q: What volume of chlorine gas at 20.0°C and 95.5 kPa is needed to produce 65.0g of HCI? H2 + Cl2 2HCI…

A: Given the chemical reaction as follows,H2+Cl2→2HClwe are to calculate the volume of chlorine gas at…

Q: A 10.0 L tank at 4.23 "C is filled with 7.60 g of chlorine pentafil gases under these conditions.…

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Q: Calculating mole fraction in a gas mixture A 9.00 L tank at 26.9 °C is filled with 11.0 g of sulfur…

A: Mass of boron trifluoride = 4.84g Mass of sulfur hexafluoride = 11.0 g    Molar Mass of boron…

Q: Ammonia gas has a molar mass approximately 17 grams per mole. At 290k and 1.2 atm a sample of…

A: Molar mass of NH3 = 17 g/mol  Temperature = 290 k  Pressure = 1.2 atm  Volume = 3.7 L  Explain how…

Q: gas. Assuming a sufficiently strong reaction vessel how much HCI (in atm) can be formed when…

A: Chlorine gas undergo free radical reaction when it is exposed UV light due to the presence of weak…

Q: Using the procedure in Experiment 8, acetonitrile (molar mass = 41.05 g/mol) is collected at a…

A: Answer:- This question is answered by using the simple concept of calculation of volume of a gas…

Q: A 7.00 L tank at 21.9 °C is filled with 5.47 g of sulfur hexafluoride gas and 5.98 g of boron…

A: Given : Volume of tank = 7.00 L Temperature = 21.9 oC Mass of sulfur hexafluoride i.e SF6 = 5.47 g…

Q: 13. If 3.5 kg of Fe is produced by the following reaction, what volume, at STP, of CO2 would be…

A: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)  Given mass Fe produced = 3.5 Kg =3500 g Number of moles of Fe…

Q: Solve the given problems. Show your solutions. 1. Calculate the volume of CO2 (g) measured at STP…

A: Concept of molar volume :- Avogadro's hypothesis states that equal volumes of all gases at the same…

Q: What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's…

A: Amount of product formed calculation using stoichiometric coefficients

Q: O STATES OF MATTER Calculating mole fraction in a gas mixture A 8.00 L tank at -3.4 °C is filled…

A: Given :-  Mass of BF3 = 9.03 g  Mass of N2O = 4.25 g  Volume of tank = 8.00 L  Temperature = -3.4°C…

Q: Calculate the volume of oxygen gas produced at 1.80 atm and 23.1°C by the complete decomposition of…

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Q: When hydrogen peroxide decomposes, oxygen is produced: 2H,0 + 0,(g)What volume of oxygen gas at 25°C…

A: Hydrogen peroxide is a chemical compound with the formula H2O2. In its pure form, it is a very pale…

Q: 12. A 6.35 gram sample of a mixture containing sodium carbonate is found to react completely with…

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Q: Calculate the volume of oxygen gas produced at STP (1 atm., 0°C) by the complete decomposition of…

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Q: What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's…

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Q: When exposed to UV light, chlorine and hydrogen gases explosively combine to form hydrogen chloride…

A: Since , PV = nRT  At constant volume and temperature  P ∝ n

Q: The concentration of gases, polluting or not, is usually expressed in ppm or ppb. Consider an air…

A: Given the concentration of SO2 in the air sample = 320 μg/m3  Temperature, T = 27+273.15 = 300.15 K…

Q: First-generation automobile airbags were inflated by the decomposition of sodium azide (M = 65.02):…

A: Ans is 2.166gg

Q: 0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative…

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Q: When exposed to UV light, chlorine and hydrogen gases explosively combine to form hydrogen chloride…

A: The expression of ideal gas equation is shown below: PV = nRT Where; P = pressure V = volume n =…

Q: How many grams of iron(III) carbonate decompose to give 67.6 mL of carbon dioxide gas at STP?…

A: Recall the reaction for decomposition of iron(III) carbonate                Fe2CO33 →∆ Fe2O3s +…

Q: Components of Air Mole Fraction Nitrogen 0.781 Oxygen 0.209 Argon 0.010 What is the partial pressure…

A: In this question, we will determine the partial pressure of Argon in torr unit.  You can see the…

Q: What is the total volume of gases produced at 1092 K and 1.00 atm pressure when 320 g of ammonium…

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Q: What is the volume in liters of hydrogen gas that would be produced by the reaction of 56.0 g of Al…

A: To calculate volume of H2 (g) , ideal gas equation is used  PV = nRT  Now number of moles of…

Q: How many litres of chlorine gas at 650 mm Hg and 25 degrees Celisus can be produced by the reaction…

A: Given,  Reaction equation: MnO2(s) + 4HCl(aq) = MnCl2(aq) + 2H2O(l) + Cl2(g) Here, 1 mol MnO2(s)…

Q: Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the…

A: Dalton's law: Dalton's law of partial pressures states that in a mixture of non-reacting gases, the…

Q: K2CO3 + 2HC2H3O3 = 2 KC2H3O2 + H2O, Find the liters of CO2 gas at STP produced by the reaction of…

A: The complete balanced reaction is shown below, K2CO3 + 2HC2H3O2 → 2 KC2H3O2 + H2O + CO2

Q: What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's…

A: The reaction involved is, C8H18 (l) + 252O2 (g)→8CO2 (g) + 9 H2O (g)

Q: To derive the ideal-gas equation, we assume that the volume of the gas atoms/molecules can be…

A: Given,The atomic radius of neon, 0.69 Å, and volume of 4πr3/3

Q: A baker uses sodium hydrogen carbonate (baking soda) asthe leavening agent in a banana-nut…

A: PV = nRT  P = 0.975 atm  T = 2000 C = 200+273 = 473 K R = 0.8206 L.atm / K mol…

Q: Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the…

A: So we will determine the mole fraction and partial pressure for Nitrogen and oxygen gas.

Q: How many liters of HNO3 will be produced from 1.00 m³ of NH3 at STP, if the concentrated nitric acid…

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.