A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.242 g of hydrogen gas. What is the percent zinc in the original mixture?

Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.042…

A: Mass of hydrogen gas produced = 1.042 g Molar Mass of hydrogen gas = 2.016 g/mol   moles of hydrogen…

Q: If 15.3 g of a particular product were obtained in a reaction and the theoretical amount was…

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Q: Acetylene gas is 92.3% carbon and 7.7% hydrogen (by mass), and its miler mass is 26 g/mol. What is…

A: A numerical problem based on molecular formula determination, which is to be accomplished.

Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.402…

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Q: what is the mass in grams of aluminum iodide that would be required to yield an actual amount of…

A: Number of moles = mass/molar mass  Mass = moles × molar mass  Percent yield = (actual…

Q: What mass of potassium would react with excess chlorine to produce 156 g of potassium chloride?

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Q: Elemental phosphorus occurs as tetratomic molecules, P4. What mass of chlorine gas is needed to…

A: Phosphorus reacts with chlorine to form phosphorus pentachloride. The equation for the balanced…

Q: What is the percentage of calcium carbonate present in the original mixture?

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Q: Mass of watch glass and evaporating dish (g) 52.08 Mass of watch glass, evaporating dish, and Mg…

A: Given- Mass of watch glass and evaporating dish = 52.08 g Mass of watch glass, evaporating dish, and…

Q: Elemental sulfur occurs as octatomic molecules, S8. What mass (g) of fluorine gas is needed to react…

A: Given- Elemental sulfur occurs as octatomic molecules, S8. 17.8 g of sulfur to form sulfur…

Q: If after heating the reaction between magnesium and hydrochloric acid, the mass of the magnesium…

A: Given: The mass of the crucible = 34.2 g The mass of the magnesium chloride formed and crucible =…

Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.372…

A: The number of moles of hydrogen (H2) gas, nH2, is; nH2=mH2MMH2=1.372 g2.016 g/mol=0.681 mol

Q: If 25.0 g of NH₃ and 45.0 g of O₂ react in the following reaction, what is the mass in grams of NO…

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Q: 34.0 g of aluminum and 39.0 g of chlorine gas, How much would be the excess reactant?

A: The molar mass of aluminium (Al) is 26.98 g/mol. The molar mass of chlorine gas (Cl2) is 70.9 g/mol.

Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.442…

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Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.092…

A: MZn + MMg = 20 g Mass of Zinc, MZn = X g Mass of magnesium, MMg = (20 – X)g Mass of Hydrogen gas =…

Q: For the following reaction, 20.9 grams of iron are allowed to react with 4.99 grams of oxygen gas .…

A: Given: Mass of Fe taken = 20.9 g. Mass of oxygen i.e. O2 taken = 4.99 g. And the reaction taking…

Q: The combustion of 0.374 kg of methane in the presence of excess oxygen produces 0.983 kg of carbon…

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Q: When 56.39 g of phosphorus pentachloride reacts with excess water, what mass of hydrogen chloride…

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Q: A 4.560 g sample containing impure CuCl2x2H2O was heated to constant mass. The sample mass after…

A: Here, impure sample of CuCl2.2H2O heated to drive off all the water then the mass of the mixture is…

Q: Elemental phosphorus occurs as tetratomic molecules, P4. What mass of chlorine gas is needed to…

A: The reaction of P4 and Cl2 is

Q: A 58.5 g sample of an unknown compound that contains only carbon, hydrogen and oxygen was analyzed…

A: Given: The mass of the unknown compound is 58.5 g The mass of CO2 (carbon dioxide) is 105.6 g The…

Q: If 45 grams of N2 are actually determined from a reaction, what is the percent yield if the…

A: Percent yield is defined as the percentage ratio of the actual yield to the theoretical yield…

Q: Aqueous sulfuric acid (H,SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous…

A: Given : mass of H2SO4 = 42.2 g mass of NaOH = 17.0 g The reaction taking place is  NaOH (aq) + H2SO4…

Q: If 18.2 kg NH3 is produced by a reaction mixture that initially contains 6.00 kg H2 and an excess of…

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Q: If 4.41g of nitrogen reacts with 2.00g of hydrogen to produce ammonia, what is the limiting reactant…

A: Given: The weight of nitrogen is 4.41 g. The weight of hydrogen is 2.00 g.

Q: 1.51 g H2 is allowed to react with 10.0 g N2, producing 2.01 g NH3 . Part A What is the theoretical…

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Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.132…

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Q: A student, Ken, is given a mixture containing two nitrate compounds. The mixture includes NaNO, and…

A: With datas given  With molar mass of NaNO3, Ca(NO3)2 ,NO3 known mass percentage of NaNO3 is done…

Q: A 3.859 g sample containing impure CuCl2· 2 H20 was heated to constant mass. The sample mass after…

A: The impure sample of CuCl2.2H2O heating to drive off all the water then the mass of the mixture is…

Q: Elemental phosphorus occurs as tetratomic molecules, P₄.What mass of chlorine gas is needed to react…

A: Given data, The weight of the phosphorus is 455 g. Then, we have to calculate the mass of chlorine.…

Q: If 27.0g of iron nail was used to react with oxygen gas, calculate the mass of ferric oxide produced…

A: Stoichiometric equation is 4Fe(S)+3O2(9) → 2Fe2O3 (s)2Fe(S)+32 O2(9) →Fe2O3 (s)2 mol     32mol…

Q: If the actual mass of a product formed in a reaction is 12.75 g less than the theoretically…

A: Given, Theoretical mass = 25.69 g Actual mass is 12.75 g less than the theoretical mass.

Q: Calculate the mass of each element in Rhenium Bromide (ReBr3) when 93.7 g of Bromine gas (Br2)…

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Q: The molecular weight of hemoglobin is about 68,000 amu. What is the mass in grams of a single…

A: The 1 amu or μ, atomic mass unit, is equivalent to 1.66×10-24 g.

Q: If 101 g of CaO and 280. g of NH4Cl are mixed, what mass of NH3 can be produced?

A: Given,CaO is 101 gAmmonium chloride is 280 gMolar mass of CaO is 56.0774 g/molMalar mass of Ammonium…

Q: If 1.36 g of Iron is heated and placed in a bottle containing 0.0198 moles of oxygen gas, what mass…

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Q: Nitrogen and Hydrogen are converted to ammonia at high temperature. When 500 g of H2 are added to…

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Q: A 12.21 g sample of a compound that contains sulfur is analyzed by precipitating all the sulfur as…

A: Given: The mass of the sample = 12.21 g The mass of BaSO4 = 11.227 g Standard data: The molar…

Q: What mass of aluminum is produced

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Q: Magnesium reacts with iron (III) chloride to form magnesium chloride and iron. A mixture of 43.5 g…

A: Given Mass of Mg = 43.5 g Mass of iron (III) chloride (FeCl3) = 173 g

Q: A 20.00 g mixture of magnesium and zinc metal reacting with excess hydrochloric acid produced 1.102…

A: Given, mass of mixture = 20.00 g Hydrogen gas produced = 1.102 g

Q: If the company chemist calculated that 12,163 g of NH3 should be produced, what is the percent…

A: Percent yield = (actual yield/theoritical yield) × 100 %

Q: Barium and sulfur react with each other in a synthesis reaction. If 0.7850 g of sulfur reacts with…

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Q: If 23 grams of iron (II) chloride reacts with 41 grams of sodium phosphate, what is the limiting…

A: Given: Mass of iron (II) chloride (FeCl2) = 23 g Mass of sodium phosphate (Na3PO4) = 41 g Molar mass…

Q: If you are provided with 10 molecules of hydrogen and 10 molecules of oxygen, which reactant is the…

A: The limiting reagent is a substance that is consumed totally when the chemical reaction is complete.…

Q: If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 17.98 g potassium oxide, what…

A: 4K + O2 ---> 2K2O Mass of K2O formed by 25 g of potassium metal  = 25 g K × (1 mol K/39.0983 g K)…

Q: In the reaction involving 2.6 g of lead (II) nitrate and 4.6 g of potassium bromide, what is the…

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Q: Barium and phosphorus react with each other in a synthesis reaction. If 0.2856 g of phosphorus…

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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.