A number of reactions can be used to generate common gases on a laboratory scale. For example, nitrogen can be produced from sodium metal and potassium nitrate as indicated by the balanced equation: 10Na(s)+2KNO3​(s)=K2​O(s)+5Na2​O(s)+N2​(g) A common laboratory-scale reaction can also generate oxygen gas by heating potassium chlorate, as indicated by the balanced equation: 2KClO3(s)=2KCl(s)+3O2(g) What mass of potassium nitrate is needed to generate 195.0  L of gas, composed of 125.0  L of N2 and 70.0  L of O2 at 0.720 atm and 299  K, using these two reactions? What mass of potassium chlorate is needed to generate 195.0 L of gas, composed of 125.0 L of N2 and 70.0 L of O2 at 0.720 atm and 299 K, using these two reactions?

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.

given the following equation 2 Co2O3(s) + 3 C(s) --> 4 Co(s) + 3 CO2(g) indicate the coefficient for elemental carbon 6 4 1 3 or 2

There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: →+2Cu2Ss  3O2g + 2Cu2Os  2SO2g In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: →+Cu2Os  Cs + 2Cus  COg Suppose the yield of the first step is 86.%  and the yield of the second step is  64.% . Calculate the mass of copper(I) sulfide required to make  2.0kg  of copper.   Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

The balanced equation for the combustion of butane, CaH1o, is shown below. 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 CAH10(g) + 13 02(g) -> 8 CO2(g) + 10 H20(1) 58.124 32 44.011 18.016 What mass of butane, in kg, will be needed to react fully with 250 L of oxygen gas?

What mass of CO2 (in Kg) does the combustion of a 12-gallon tank of gasoline release into the atmosphere? Assume the gasoline is pure octane (C8H18) and that it has density of 0.70 g/mL. You will need a balanced chemical equation for combustion of octane.

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3  and water:   2Al(OH)3(s) + Al2O3(s) ->  3H2O(g) In the second step, alumina Al2O3  and carbon react to form aluminum and carbon dioxide:   2Al2O3(s) +  3C(s) + 4Al(s) ->  3CO2(g) Suppose the yield of the first step is 74.%  and the yield of the second step is  76.% . Calculate the mass of aluminum hydroxide required to make  4.0kg  of aluminum.   Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

Aqueous iron(II) sulfate (FeSO4) and solid copper are produced by the reaction of solid iron and aqueous copper(II) sulfate (CuSO4). Write a balanced chemical equation for this reaction. □ X Ś