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Consider the reaction: C2H4 + O2     →     CO) (Unbalanced).  If 0.96 g of C2H4 g was Used 5.2 g of CO2 produced, calculate the percentage yield in the reaction. (Hint Balance the equation first).

A container holds 75.0 g of CuO and 5.00 g of H₂. The following reaction occurs: CuO + H₂ --> Cu + H₂O. What is the theoretical yield of Cu that can form?

Potassium perchlorate, KClO4, is a better oxidizing agent than the potassium chlorate, KClO3, described in the previous problem. Potassium perchlorate, which is used in explosives, fireworks, flares, and solid rocket propellants, is made by carefully heating potassium chlorate to between 400 °C and 500 °C. The unbalanced equation for this reaction is KClO3 → KClO4 + KCl Balance this equation. Write a conversion factor that could be used to convert between moles of potassium chlorate and moles of potassium perchlorate. How many moles of potassium perchlorate form from the complete reaction of 12 moles of potassium chlorate? Write a conversion factor that could be used to convert between moles of potassium perchlorate and moles of potassium chloride. How many moles of potassium chloride form along with 11.875 moles of potassium perchlorate?

If you start with a mixture of Nacl and KClO3 that weighs 3.00g, and the mass of the sample decreased by 0.75g after heating, what is the best explanation for the change in mass? -0.75g KClO3 and NaCl reacted to form products -0.75g O2 was formed in the reaction and left the same sample as gas -0.75g KCl was formed -0.75g KClO3 reacted to form products or.. -0.75g NaCl reacted to form products

Balance the following chemical reaction and determine the number of moles of HI produced when 2 moles of H2(g) are consumed in the following chemical reaction: H2(g) +l2(g) →__HI(g)

6. Consider the reaction: 2Sb(s) + 312(s) → 2Sbl3(s). Determine the limiting reactant and the theoretical yield when 1.20g of Sb and 2.4g of lz are mixed? What mass of the excess reactant is left when the reaction is complete?

100 g manganese dioxide reacts with 300g hydrochloric acid in the reaction shown bellow. MnO2 + 4 HCl -> 2 H2O + Cl2 use the following molar masses: MnO2 = 86.9g HCl = 36.5g MnCl2= 125.8g H2O= 18.02g Cl2= 70.9g 1.) Which reactant is limiting? 2) Which reactant is excess? 3) What is the theoretical yield of Cl2?

An initial reaction mixture contains 9.42 g of Fe and 8.50 g of S. The following reaction occurs: Fe(s) + S(s) → FeS(s) a) Calculate the theoretical yield of FeS. b) How much of the excess reactant remains unreacted?

5. Consider the following reaction:           BaCl2(aq)  +  2 AgNO3(aq)  -->  2 AgCl(s)  +  Ba(NO3)2(aq) How many moles of BaCl2 are needed to prepare 61.30 moles of AgCl?