Fe + H20)→ Fez04(s) + H ²(ø) a. How many moles of Fe would be required to react with 2.0 mol of H20?

Q: Calculate the number of grams of bromine (Br2) needed to react exactly with 50.1 g aluminium (Al).…

A: Mass of aluminium (Al) = 50.1 g The balanced equation given is, 2 Al (s) + 3 Br2 (l)  → 2 AlBr3 (s)

Q: Vanadium (V) oxide is decomposed into the elements sodium and chlorine by means of electrical…

A: 2V2O5 --> 4V  + 5O2 this oxygen oxidises sulphur to sulphur dioxide 5S  +   5O2 --> 5SO2  five…

Q: The metals industry was a major source of air pollution years ago. One common process involved…

A: Given the reaction is, 2PbS+3O2---->2PbO+2SO2 Mole of PbS is 9.53mol. We have to calculate mole…

Q: O₂(g) + 2 H₂(g) → 2 H₂O(1) - Assume 0.250 mol O₂ and 0.810 mol H₂ are present initially. After the…

A: The stoichiometry of the balanced chemical reaction states that one mole of oxygen reacts with two…

Q: What is the mass in grams of NO that will be produced from 51.8 g of NO₂ reacted with excess water…

A: For determining the amount of product, the mole ratio of reactants in a balanced reaction must be…

Q: CH4(g)+2O2(g)→CO2(g)+2H2O(g) What mass of water is produced from the complete combustion of…

A: The objective of the question is to find out the mass of water produced from the complete combustion…

Q: I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation:…

A:

Q: How many grams of NO will be produced from 76.2 g of NO₂ reacted with excess water in the following…

A:

Q: How many moles of O₂ are required to produce 2.50 mol of CO₂?

A: The reaction between carbon and  O₂ to produce CO₂ is as follows: C + O2 ---> CO2

Q: A piece of magnesium with a mass of 0.0501 grams was placed into a solution containing an excess of…

A: The balanced reaction taking place is given as, => Mg (s) + 2 HCl (aq) ------> MgCl2 (aq) + H2…

Q: What is the mass in grams of NO that will be produced from 10.7 g of NO₂

A: Given :- 3 NO₂(g) + H₂O(l) → 2 HNO₃(g) + NO(g)                Mass of NO2 = 10.7 g  To calculate :-…

Q: Use the balanced equation, 4K + O₂ 2 K₂O, to answer the following question. How many grams of K are…

A: mass of O2 = 19.1 gmolar mass of O2 = 32.00 g/molAtomic mass of K = 39.10 g/mol

Q: Ammonia is manufactured using the following reaction: n2 + 3h2 → 2nh3 How much ammonia can be…

A: Given, Moles of N2 = 2.04 × 10-3 mol Moles of H2 = 6.83 × 10-3 mol

Q: Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce…

A: Nitrogen reacts with hydrogen to form ammonia. The equation for the balanced chemical reaction is…

Q: How many grams of chlorine gas can be produced from the decomposition of 73.4 g. of AuCl3 by this…

A: The formula used for calculating the number of moles is as- no. of moles (n)= massmolecular weight…

Q: Fe₂O₃(s) + Al(s) → Fe(l) + Al₂O₃(s) calculate the moles of Fe₂O₃ that will be required to produce…

A: The balanced chemical equation for the reaction between Fe2O3 and Al is: Fe2O3(s) + 2Al(s) → 2Fe(l)…

Q: The combustion of propane (C3H8 ) in the presence of excess oxygen yields CO2 and H2O: C3H8 (g) +…

A: (a) Propane is an alkane with the molecular formula C3.H8, which has 3 carbons and 8 hydrogen…

Q: What mass of aluminium oxide formed when 10.0g of Al is burned in 20.0g of O2?

A: Given: The amount of Al = 10.00 g The amount of O2 = 20.00 g Al burns in O2 to given an oxide of Al…

Q: Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2(s) +…

A: The given reaction is    SrH2s+2H2O→SrOH2l+2H2g   mass of SrH2 is given by mSrH2=2.81g   mass of…

Q: What mass of Carbon dioxide is produced by the complete combustion of 100 g of the hydrocarbon…

A: Using stoichiometric calculations, we will calculate mass of CO2 produced.

Q: What mass in grams of the dihydrate H2C2O4 • 2 H2O (molar mass = 126.0 g/mol) is needed in order to…

A: The dihydrate H2C2O4 • 2 H2O losses two equivalent of water molecules to form H2C2O4  in the…

Q: Lithium hydroxide is frequently used to neutralize sulfuric acid according to the equation: 2LiOH +…

A:

Q: Consider the oxidation of sodium metal to sodium oxide described by the balanced equation:…

A: Given, the mass of the Na = 2.55 g  the mass of the O2 = 1.98 g The chemical reaction of sodium…

Q: How many moles of Al are necessary to form 71.2 g of AIBR, from this reaction: 2 Al(s) + 3 Br,(1) –→…

A:

Q: How many moles of glucose can be formed from 2.53 × 1024 H atoms?

A:

Q: How many moles of sodium chlorate (NaCIO3) are required to produce 0.235 mol O2? 2 NaCIO3(s) – 2…

A:

Q: What mass of O2 can be generated by the decomposition of 100.0 g of NaClO3? 2 NaClO3 → 2 NaCl(s) + 3…

A: Given, The balance chemical equation, 2 NaClO3 → 2 NaCl(s) + 3 O2(g)  The mass of NaClO3 = 100 g To…

Q: How many moles of O₂ can be formed from 5.5 moles of KClO₃ in this equation? 2KClO₃(s) → 2KCl(s) +…

A:

Q: 2. Most commercial hydrochloric acid is prepared by heating NaCl with concentrated H₂SO4. How much…

A:

Q: Calculate the percent yield of Cl2 (g) in the electrolytic decomposition of hydrogen chloride (HCl)…

A: The percentage yield can be calculated with the help of theoretical and experimental yield.

Q: How many grams of carbon dioxide would be required to react with 51.2 g of LiOH in the following…

A: Chemical Reaction :  2 LiOH(s) + CO₂ (g) → Li₂CO₃ (s) + H₂O (l) Mass of LiOH = 51.2 g  Mass of CO2 =…

Q: Ethanol (C,H,O) is combusted in air according to the following reaction: C,H,O(1) + 0,(g) → CO,.(g)…

A: Combustion Reaction :- When an organic molecule reacts with oxygen it produces water  vapor and…

Q: How many moles of Al are necessary to form 48.0 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) →…

A:

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.