Water can be broken down via electrolysis according to the reaction, 2 H2O (l) --> 2 H2 (g) + O2 (g) Calculate the pressure exerted by O2 when 4.721  g of water is completely broken down and the gases are collected in a 1.947 L container at 25 oC.  Hint: calculate the number of moles of O2 produced first.

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Q: When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon…

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Q: CH3OH can be synthesized by the following reaction. CO(g)+2H2(g)→CH3OH(g) What volume of H2 gas (in…

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Q: 8.00 gram mixture of copper (II) sulfide and iron (II) sulfide reacted with excess nitric acid and…

A: Given the mass of mixture = 8.00 g composition of mixture is copper (II) sulfide, CuS(s) and iron…

Q: A sample of O2 with a pressure of 1.53 atm and a volume of 239 mL is allowed to react with excess NO…

A: The combined gas law is given by

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Q: The combustion of octane, C,H18, proceeds according to the reaction shown. 2 C3H18(1) + 25 0,(g) –…

A: The balance chemical reaction :  2C8H18(L) + 25O2(g) ----> 16CO2(g) + 18H2O(L)  Number of moles…

Q: Gaseous ammonia and hydrogen chloride react to form solid ammonium chloride, NH3 (g) + HCI (g) →…

A: Calculate the excess moles of reactant,         Moles of NH3 = 3.00 g17.031 g/mol = 0.1761 molMoles…

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A: Here we are required to find the mass percentage of Al in the sample.

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A: The reaction taking place between is,

Q: 3 H2 (g) + N2 (g) --> 2 NH3 (g)   A 3.22 L vessel containing the hydrogen at 21.1 oC and 6.750 atm…

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Q: A steel tank has a volume of 438 L and is filled with 0.885 kg of O2. Calculate the pressure of O2…

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Q: Calculate the pressure exerted by O2 when 1.181  g of water is completely broken down and the gases…

A:

Q: The combustion of octane, C,H,18, proceeds according to the reaction shown. 2 C,H,(1) +25 0,(g) 16…

A:

Q: 5.41 A sample of a smokestack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed.…

A: For 100 g sample, Mass of CO2 = 92 g Mass of NO = 3.6 g Mass of SO2 = 1.2 g Mass of water = 4.1 g

Q: For the balanced reaction below, what volume of nitrogen monoxide gas would be required to…

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Q: A 4.07 L volume of oxygen gas measured at 4.94 °C is expanded to a new volume of 4.50 L. Calculate…

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Q: 42. What mass of KCIO, will produce 250 mL of O2 gas, collected by water displacement, at an…

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Q: Both Jacques Charles and Joseph Louis Guy-Lussac were avidballoonists. In his original flight in…

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Q: The reaction: 2NaN3(s) → 2Na(s) + 3N2(g), have sodium azide (NaN3) used in some automobile air bags.…

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Q: CH3OH can be synthesized by the following reaction.CO(g)+2H2(g)→CH3OH(g) What volume of H2 gas (in…

A: According to the question, methanol is prepared by the given reaction.From this reaction, 2 moles of…

Q: The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine…

A:

Q: What volume of oxygen gas is produced when 29.4 g of mercury(II) oxide reacts completely according…

A: The given chemical equation is: 2 HgO (s) → 2 Hg (l) + O2 (g) Given mass of HgO = 29.4 g  Molar mass…

Q: Nitrogen and hydrogen react in the Haber process to form ammonia. All substances are in the gas…

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Q: The combustion of octane, C, H,8. proceeds according to the reaction shown. 2C,H,,(1) + 250,(g) - 16…

A:

Q: How many moles of nitrogen will be needed to react with 1.5 L of H₂ gas measured at 20°C and 0.95…

A:

Q: The combustion of octane, C,H, proceeds according to the reaction shown. 18 2C,H18(0) + 25 0,(g) 16…

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Q: Consider the following equation: C6H8O7(s)  + 3 NaHCO3(s) + H2O(l) --> Na3C6H8O7(s) + 3H2O(l) +…

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Q: When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al(s) + 6…

A: The balanced chemical reaction of aluminium with hydrochloric acid at STP to produce aluminium…

Q: In a combustion reaction, what mass of oxygen gas is needed to react with 25.0 mL of C4H10 gas,…

A: Given :-  Volume of C4H10 gas at STP = 25.0 mL  To calculate :-  Mass of O2 (in grams)

Q: ulfur burns in oxygen with a deep blue flame to produce sulfur dioxide.  If 5.85 g S8 and 1.00 atm…

A: Given : Mass of  S8 = 5.85 g  Pressure of 02 = 1 atm Volume = 5.00 L

Q: Roasting galena [lead(II) sulfide] is an early step in the in-dustrial isolation of lead. How many…

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Q: A 280ml container of chlorine gas kept at 25C and 746 torr is exposed to 1.25g white phosphorus (P4)…

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Q: CH3OH can be synthesized by the reaction:CO(g) + 2 H2(g) --------> CH3OH(g)What volume of H2 gas…

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Q: Consider the reaction of NO2  If 23.8L of O2(g), measured at 35oC and 632mmHg is allowed to react…

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Q: 4) Given these reactants and products: NH3 + Cl, ---> N, + HCI Balance the chemical equation. How…

A:

Q: 4 NH3 (g) + 5 O2 (g) = 4 NO (g) + 6 H2O (g)A sample of NH3 is added to an initially evacuated 2.00 L…

A: Given dataPartial pressure of NH3= 415torrPartial pressure of O2 = (875-415) torr…

Q: Fat is a complicated mixture but has the approximate formula of C56H10806- Consider the following…

A:

Q: 1. A student neglected to keep the end of the delivery tube under the surface of the water displaced…

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Q: The combustion of octane, C,H,2, proceeds according to the reaction shown. 2C,H18() + 25 0,(g)16…

A: 2 moles of octane give 16 moles of CO2. So, 354 mol of octane will give (8*354) = 2832 mol of CO2.…

Q: The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine…

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Q: A sample of H, with a pressure of 1.89 atm and a volume of 274 mL is allowed to react with excess N2…

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Q: Calculate the volume of C3H8 gas produced from the reaction of 17.1 liters of CO gas with excess…

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Q: collected in a reaction where 215mL of oxygen gas is collected over water at a temperature of 25 ∘C…

A: We will use ideal gas equation to get the answer.

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.