Calculate the mass of excess reagent (in grams) remaining at the end of the reactjon in which 90.0 g of SO2 are mixed with 100.0 g of O2. 2SO2 + O2 --> 2SO3

Q: What amount (in mol) and what mass (in g) of water can be produced when 82.1 ug of ethane reacts…

A: The reaction considered is, C2H6 (g) + O2(g)→H2O(l)+CO2(g) The balanced equation of this reaction…

Q: 2KCIO3 → 2KCI + 302 What is the total number of moles of KCIO3 needed to produce 6 moles of O2? O 1…

A: Answer :- Option B is correct answer. (I.e., 4 Mole of KClO3 )

Q: Calculate (a) the number of moles of potassium dichromate (K2Cr2O7) that will react with 2.0 moles…

A: Given reaction,     K2Cr2O7+KI+H2SO4  → Cr2(SO4)3+K2SO4+I2+H2O

Q: Give the percent yield when 28.16 g of CO, are formed from the reaction of 4.000 moles of C3H18 with…

A: We have to calculate the percentage yield.

Q: 4. A mixture of 3.00 g of Bi₂03 and 0.500 g C are used to produce bismuth and CO in the reaction…

A: The given balanced chemical react between Bi2O3 and Carbon is        Bi2O3 + 3 C ------> 2 Bi +…

Q: cetic Acid Aspirin 1on se 0 ag nol) 1stbo nn sved nenonbyil nedt 1adio 2mole e in Consider the…

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Q: Give the theoretical yield, in moles, of CO2 from the reaction of 0.60 moles of C8H18 with 40.00…

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Q: Determine the limiting reagent if 2.2g of Mg is reacted with 4.5L of Oxygen (Standard Temperature…

A: Given, 2Mg(s) + O2(g) -> 2MgO(s) Mass of Mg reacts = 2.2 g Volume of Oxygen gas reacts =4.5 L…

Q: How many moles of Cr2O3 will form when 0.35 moles of Cr is mixed with 0.25 moles of O2?

A: Since you have posted a  question with sub-parts , we are entitled to answer the first three…

Q: Overall reaction: Nal NaOCl NH2 OH compound salicylamide sodium OH NH2 NaOCl (15 iodosalicylamide…

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Q: The traditional way of comparing reactions is by the percentage yields. However, percentage yield…

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Q: Consider the following balanced reaction. How many moles of C3H7SH  are need to produce 0.224 moles…

A: The term number of moles is defined as the ratio of mass to the molar mass of the given compound.…

Q: Determine the moles of HCI produced when 36.1 grams of Cl, reacts with H, according to the following…

A:

Q: How many grams of NO will be produced from 31.3 g of NO2 reacted with excess water in the following…

A: First convert the mass of NO2 into moles. Then by using moles of NO2 and Balanced chemical equation…

Q: LI3OCI (a solid electrolyte in lithium ion batteries) can be prepared as shown below. LICI 2 LİOH…

A: The amount of a product formed in a chemical reaction is determined by the limiting reagent. The…

Q: have a question about theoretical yield. I know we are supposed to always start with the limiting…

A: If both the reactant are limiting that is completely consumed either one of them can be used to…

Q: Consider the reaction of a 20.0 mL of 0.220 M C H NHCI (Ka = 5.9 x 10) with 12.0 mL of 0.231 M CSOH.…

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Q: Amounts starting materials used in lab and calculation of moles 2-methylcyclohexanol (g) 85%…

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Q: Calculate the number of moles of Fe3O4 produced from 7.42 moles of Fe by the following balanced…

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Q: A sample of baking soda, NaHCO3, is decomposed while releasing steam and carbon dioxide gas as…

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Q: Calculate the number of moles of Na2CS3 produced from 1.34 moles of NaOH by the following reaction.…

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Q: Bod 44 grams of carbon dioxide was formed after combustion of 12 grams methane gas. Calculate…

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Q: N2 + 2O2 -> N2O4 If you mix 1.3 mol of N2 and 2.3 mol of O2, which is the limiting reagent?

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Q: 5. The combustion of glucose is represented by the following balanced equation: C6H12O6 +6 026 H₂O +…

A: Reaction-C6H12O6 +6O2 6H2O +6CO2Mass of C6H12O6 =1gMass of O2 = 1gMolar mass of C6H12O6 =…

Q: O what ave The products from the to dauble-replacement reaction ? AgNOGag) +kgPDy laq)

A: In a double displacement reaction, the counter ions of two reactants get exchanged to give two new…

Q: Give the percent yield when 28.16 g of CO_2[/math} are formed from the reaction of 4.000 moles of…

A: Interpretation-  To determine the percentage yield of 28.16 g of CO2 in the given reaction that is -…

Q: What is the percent atom economy and the E-factor for the reaction below?    3 CO + 7 H2 ⟶  C3H8 +…

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Q: Would it affect your calculation of theoretical yield? Could it affect your measurement of actual…

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Q: What mass of FeS is required to produce 87g Fe2O3 with excess O2 by this reaction 4FeS + 7 O2 —>…

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Q: E-85 is an alternative fuel for automobiles and light trucks that consists of 85.0% (by volume)…

A: Given balanced equation:

Q: If you are given 1.35g Fe(NO3)3 and 0.00597 mol of Cl2 to conduct the gas forming reaction below…

A: Given mass of Fe(NO3)3 = 1.35g Moles of Cl2 = 0.00597 molGiven balanced reaction: 2Fe(NO3)3 + 2Cl2 →…

Q: Given the following reaction: 2 Al + 2 KOH + 4 H2SO4 +22 H20-- 3 H2 + 2KAI(SO2 12H20 If you start…

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Q: For this reaction, 2 NH3 + CO2 --> H2NCONH2 + H2O how many moles of CO2 are required to produce 3.0…

A: The balanced equation is:  2 NH3 + CO2 --> H2NCONH2 + H2O It is shown that 2 mol of NH3 react…

Q: 4. Consider the reaction MnO2 + 4HCI → MnCl2 + Cl2 + H20 If 86.3 L of MnO2 and 48.2 L of HCl react,…

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Q: I need help with questions 2-5 with guided steps.... I only got help with the first one which I…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Calculate the mass of excess reagent (in grams) remaining at the end of the reaction in which 90.0 g…

A:

Q: If exactly 4.089 moles of propanol (C3H8O)  is combusted in the presence of excess oxygen what is…

A: Given data: The moles of propanol combusted is 4.089 mol. To calculate: The mass of O2 was used in…

Q: for the reaction: 2 NaHCO3 → Na₂CO₂ + H₂O + CO₂ Find the mass of Sodium Carbmate that reacted from…

A: Given : mass of sodium bicarbonate = 1.56 g

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".