A mixture of C3H8 and C2H2 has a mass of 2.4 g . It is burned in excess O2 to form a mixture of water and carbon dioxide that contains 1.6 times as many moles of CO2 as of water. Find the mass of C2H2C2H2 in the original mixture. Express your answer to two significant figures and include the appropriate units

Product Composition and Reaction Stoichiometry Suppose SH2 and O2 react to produce H20, and a sulfur oxide which contains 40.05% sulfur by mass. Complete the reaction equation by entering the coefficients of the reactants and products and also the empirical formula of the sulfur oxide product. SH2 + H20 + All coefficients must be reduced to the smallest possible integers. Note that, while it is not usual to write coefficients of exactly 1, you must enter "1" in the response box, if that is the correct value. The formula for the sulfur oxide must be written with the S symbol first and O second. The usual subscription of numbers in the formula is to be inferred (e.g. the formula for water would be entered simply as "H2O")

Iron reacts with oxygen gas to form a mixture of FeO and Fe₂O₃ when the supply of oxygen is regulated. A sample of 20.00 g iron metal reacts with oxygen gas to form 28.10 g iron oxide mixture, and all of the iron metal was consumed. What is the mass in g of FeO that were produced in the mixture?

4. Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. (i) Determine whether the data given confirm the formula of the hydrate. You must (ii) show any relevant calculations that support your answer.

A mixture of C3H8C3H8 and C2H2C2H2 has a mass of 2.7 gg . It is burned in excess O2O2 to form a mixture of water and carbon dioxide that contains 1.6 times as many moles of CO2CO2 as of water. Find the mass of C2H2C2H2 in the original mixture. Express your answer to two significant figures and include the appropriate units.   mC2H2=

Tristearin C 57H 11006), obtained from animal fats, was historically used as a household fuel source. The burning of tristearin is depicted as: 0,+0,−CO,+H,0 2 CH 57 110 6 2 When 5.79 kg of tristearin and pure oxygen gas at 9.30% excess were reacted, 11.29 kg of CO2 is recovered. Determine the percent yield of CO2. Type your answer as a percent, 2 decimal places.

3.275 g of potassium bitartrate (KH5C4O6(s) are suspended in water and reacted with sodium carbonate (Na2CO3). How many grams of sodium carbonate are neeeded to react with this much potassium bitartrate. 2KH5C4O6(s)+Na2CO3(s)+3H2O(l)>CO2(g)+2NaKH4C4O6*4H2O(s). Potassium bitartrate MM=188.18g/mol ROCHELLE SALT MM =282.22g/mol sodium carbonate MM= 105.99 g/mol

Consider the haber-bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH3 from the complete reaction of 15.6 grams H2 in the presence of excess N2 gas according to the following balanced chemical equation. N2(g) + 3H2(g) -> 2NH3(g)

bctions: Show your solution in the space provided. Follow the GFFSA (Given, Find, ymula, Solution, Answer) format if possible. Write your answers in the space provided. 1. Combustion of hydrocarbons like methane (CH4) produces two products, water (H2O) and carbon dioxide (CO2). Consider the chemical equation of this combustion: CHA + 2 02 - CO2 + 2 H2O, when 4 mol of CH4 reacts with 4 mol of O2, how many moles of CO2 are formed? What is the limiting reactant? 2. How many grams of lead II chloride are produced from the reaction of 16.2 g of NaCl and 62.0 g of Pb(NO3)27 What is the limiting reactant? How much excess is left over?

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