Magnesium reacts with oxygen to produce magnesium oxide. If 2.851 grams of magnesium reacts with excess oxygen to produce 3.475 grams of magnesium oxide, what is the % yield for the reaction?

Q: calculate the mass of water that forms when 2.00 grams of hydrogen peroxide decompose. Molecular…

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Q: what mass of H2O is produced in this equation by 9.91 grams of ammonia

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Q: A student is given a 1.8686 g of an unknown copper compound. Following isolation by displacement by…

A: Given: Mass of Cu = 0.3685 g Mass of compound = 1.8686 g

Q: What is the theoretical yield of MgO from the combustion of 5.25 x 10^23 atoms of Mg and 4.69 x…

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Q: What is the mass percentage of O in CO₂? Provide an answer to two decimal places.

A: Molecular weight of C and O are 12.0107 gm/mol and 15.999 gm/mol respectively.  Hence, molecular…

Q: A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When…

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Q: [2]  a. Write the balanced chemical equation for the reaction. b. Calculate for the mass of…

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Q: 2.) 350 g of Calcium Chromate reacts with excess Hydrogen Peroxide. Write a balanced chemical…

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Q: and

A: The balanced chemical reaction between CaCO3 and HCl as well as MgCO3 and HCl: Reaction 01: CaCO3 +…

Q: A 2.500g sample of an unknown hydrocarbon (CxHyOz) is put in a combustion chamber. From the…

A: We have to calculate the mass of O .

Q: Hydrogen peroxide ( H 2 O 2 ) decomposes to produce water and oxygen.Write a balanced chemical…

A: BALANCED EQUATION IS BELOW :

Q: If the solubility ofa gas in water is 0.010 gL-at 25 °C with the partial pressure of the gas over…

A: For this problem, using appropriate equation Henry's law  to solve this problem. C1/P1=C2/P2 where C…

Q: The following reaction describes the production of elemental sulfur. Calculate the mass of elemental…

A: Given- Weight of dihydrogen sulphide =15.39 g  H2S(g)+O2(g) -> S8(s) + H2O(g)

Q: If 71.0 g of Fe2O3 react with 26.9 g of Al, how much molten Fe can be formed

A: Stoichiometry, in balanced chemical reaction is defined by the ratio at which reactants are reacting…

Q: What is the mass percentage of O in CO2? Provide an answer to two decimal places.

A: Given,  The mass percentage of O in CO2 is:

Q: A 2.86 g sample of a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was…

A: Given, mass of 2.86 g sample of a compound produced 1.61 g CO2 and 0.989 g H2O.Moles of CO2 and H2O…

Q: Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced…

A: Given information,        1.40 × 103 g N24.60 × 102 g H2

Q: A mixture of C2H2 and CH4 has a total mass of 251.8 g. When this mixture reacts completely with…

A: Given:Total mass of mixture of C2H2 and CH4 = 251.8 g.Total mass of CO2 and H2O = 1138.0 g.Molar…

Q: What is the lowest possible coefficient of hydrofluoric acid in the balanced chemical equation…

A: The balanced chemical equation for the reaction of sulfur tetrafluoride with water to produce…

Q: When 4.68 g of iron is reacted with excess oxygen, 6.70 g of product is obtained. Determine the…

A: A compound contains 40% carbon, 6.7% hydrogen, and 53.3%oxygen. 100 g of the compound will contain…

Q: How many grams of oxygen are formed, if 1.0 g of H2O is decomposed per the equation below : 2H2O 2H…

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Q: What is the theoretical yield of aluminum oxide if 2.00 mol of aluminum metal is exposed to 1,80 mol…

A: Answer: This question is based on the concept of limiting reagent. Limiting reagent is the reactant…

Q: If 6.8 g of a hydrocarbon that is 83.2% C by mass is burned with O2 to make CO2 and H2O,  what mass…

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Q: 3.15 X 1023 molecules of water were collected in a distillation flask. How many moles of H20 were…

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Q: What is the percent by mass of KClO3 in the original mixture

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Q: What mass of hydrogen peroxide (H2O2) must decompose to produce 65.88 g of H2O?

A: Given data: The mass of H2O = 65.88 g. To find: The mass of hydrogen peroxide (H2O2).

Q: If 6 moles of Si and 6 moles of N2 are combined in a reaction flask, what remains in the reaction…

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Q: s. How much O2 could be produced

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Q: A 0.8102-g sample of impure Al2(CO3)3 decomposed with HCl; the liberated CO2 was collected on…

A: The percentage of Aluminum in the sample can be calculated as follows

Q: For this problem, identify the limiting reagent and calculate the grams of NaAl(OH)4obtained in the…

A: A limiting reagent is defined as the reagent that is completely consumed in the reaction and limits…

Q: A three-step process for producing molten iron metal from Fe203 is: 1. 3FE203 + CO –→ 2FE304 + CO2…

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Q: 1) Methane (CH4) combusts in oxygen to yield gaseous carbon dioxide and water vapor. Write the…

A: " Dear student , as you posted multiple different questions , as per guidelines we answer first…

Q: According to the following reaction, how many grams of mercury will be formed upon the complete…

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Q: Mesitylene is a liquid hydrocarbon. Burning 0.795 g of the compound in oxygen gives 2.62 g of CO2…

A: Given:…

Q: For the reaction N, + 3H, 2NH, what is the Mole ratio of nitrogen to hydrogen? t. Mole ratio of…

A: In a balanced chemical equation , the stoichiometric coefficients of reactants and products…

Q: How many grams of carbon dioxide can be produced by burning 1.72 moles of propane? Assume that…

A: Propane reacts with oxygen to form carbon dioxide and water. The equation for the balanced chemical…

Q: How many grams of carbon dioxide can form when a mixture of 5.00 grams ethylene and 5.70 grams of…

A: Combustion is the process of burning in aerobic  condition . Products of combustion are water and…

Q: Abel reacts copper with silver nitrate and recovers 5.2 g Ag. However, after mass to mass…

A: The theoretical yield of silver is = 9.5 g The actual yield of the silver in the reaction is = 5.2 g…

Q: hydrogen peroxide H2O2 (in grams)

A: Given : 8.00 g of oxygen gas and 0.504 g of hydrogen gas

Q: percentage by mass of calcium

A: Mass percentage of any component in a compound is calculated by formula :  Mass % = Mass of…

Q: How many moles of electrons are required to produce 18.1 g of potassium metal from a sample of…

A: We are hereby asked that how many moles of electrons are required to produce 18.1 g of potassium…

Q: Calculate the mass, in grams, of 0.433 mol of CO2.

A: Mass in grams from moles can be calculated by using the formula given below as; Mass=moles…

Q: This reaction makes potassium superaxide useful in a self-contained breathing apparatus. How much Oz…

A: First calculate moles of KO2 and CO2. Then use mol to mol ratio to check which compound forms less…