Before the use of CFCs, sulfur dioxide was used as a refrigerant.  A sample of sulfur dioxide undergoes a simple decomposition reaction as follows: 8 SO2(g) --> S8(s)  +  8 O2(g) Calculate the number of moles of oxygen gas produced in addition to the production of 1.18 mol of sulfur.

The  theoretical yield of reactions Consider the reaction 1CO(g) + O2 (g) --> 2CO2(g) if 9.420 g CO is mixed with 16.84g O2, CALCULATE THE THEORETICAL YIELD (g) of CO2 produced by the reaction.

Hydrocarbons such as propane burn in oxygen gas to produce heat. The balanced equation below shows the complete combustion of propane in oxygen. C3H₂(g) +50₂(g) → 3C0₂(g) + 4H₂O(g) How many moles of O₂ would be needed to cause the complete combustion of 3.00 g C3H8? moles

Consider the combustion reaction for octane (C,H2), which is a primary component of gasoline. 18 2 C3H13 + 25 0, → 16 CO, + 18 H,O How many moles of CO, are emitted into the atmosphere when 20.1 g C,H13 is burned? CO2 emitted: mol CO2

Write a balanced chemical equation based on the following description: butane gas reacts with oxygen gas to produce carbon dioxide gas and water vapor C4H10(g)+O2(g)_

Hydrazine (N2H4) can be synthesized from ammonia (NH3) and hydrogen peroxide (H2O2) in the Peroxide process. The balanced chemical equation of this reaction is shown below: H2O2 (l) + 2NH3 (l) → 2H2O (l) + N2H4 (l) If 4 moles of ammonia were mixed with an excess amount of hydrogen peroxide, how many moles of hydrazine would be produced?

Lead ions can be precipitated from solution with KCl according to the reaction: Pb2+ (aq) + 2KCl(aq) → PbCl₂ (s) + 2K+ (aq) When 34.3 g KCl is added to a solution containing 25.8 g Pb²+, PbCl2 (s) forms. The solid is filtered and dried and found to have a mass of 30.9 g. theoretical yield of PbCl2 = 25.8 g Ph Part C % yield = Determine the percent yield for the reaction. Express your answer in percent to three significant figures. 15 ΑΣΦ X Ċ 1 mel P5²+ 1 mol 1 met X 207.2 g Pb² ? %

The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. For your convenience, the molar mass of each substance Is shown below their formulas (in purple). Use this Information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 2900 mg of potassium chlorate:

The coefficients in a balanced chemical equation provide the mole-to- mole stoichiometry among the reactants and products. The molar mass (in g/mol) can be used as the conversion factor between moles and the mass of a substance. Thus, the balanced equation and molar masses can be used in conjunction with one another to calculate the masses involved in a reaction. Complete combustion of methane When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH₂(g) + O₂(g) →CO₂(g) + H₂O(g) This type of reaction is referred to as a complete combustion reaction. Review Constants Perio Part A What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H₂O, respectively. Express your answer as four integers, separated by commas (e.g., 1,2,3,4).

2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol   NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.