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Percent Yield

Q. For the following reaction, 5.73 grams of sulfur are mixed with excess carbon monoxide. The reaction yields 7.60 grams of sulfur dioxide. sulfur (s) + carbon monoxide (g) → sulfur dioxide (g) + carbon (s) What is the theoretical yield of sulfur dioxide? _____ grams What is the percent yield of sulfur dioxide? ____ %

Solved • Feb 4, 2020

Percent Yield

Q. For the following reaction, 4.65 grams of oxygen gas are mixed with excess carbon (graphite). The reaction yields 5.07 grams of carbon dioxide. carbon (graphite) (s) + oxygen (g) → carbon dioxide (g) What is the theoretical yield of carbon dioxide? _____ grams What is the percent yield for this reaction? ____ %

Solved • Feb 4, 2020

Percent Yield

Q. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of the experiment, their product weighs 2.41 g. What is the theoretical yield, actual yield and percent yield?

Solved • Feb 4, 2020

Percent Yield

Q. The combination of 75.00 g of Ca(OH)2 (MW 74.093 g/mol) with 200.00 mL of 4.575 M Na2(PO4)3 (MW 163.94 g/mol) solution produces 75.00 g of Ca3(PO4)2 (MW 310.17 g/mol) via the balanced chemical equation below. What is the percent yield? 3 Ca(OH)2(s) + 2 Na3PO4(aq) → Ca3(PO4)2(s) + 6 NaOH(aq)

Solved • Jan 12, 2020

Percent Yield

Q. If 15.0 g N2 and 2.00 g H2 react to produce 1.38 g NH3, what is the percent yield of the reaction? N2(g)+3 H2(g)---> 2 NH3(g)

Solved • Dec 17, 2019

Percent Yield

Q. Consider the balanced equation for the following reaction: 3Ca(ClO3)2(aq) + 2Li3PO4(aq) → Ca3(PO4)2(s) + 6LiClO3(aq) Determine the percent yield of LiClO3(aq) if 8.30 moles of Ca(ClO3)2(aq) reacts with an excess of Li3PO4(aq) and 12.3 moles of LiClO3(aq) is formed. 79.2% 54.8% 64.4% 55.5% 74.0%

Solved • Dec 11, 2019

Percent Yield

Q. Consider the balanced equation for the following reaction: 8O2(g) + C5H12(l) → 5CO2(g) + 6H2O(l) If 37.0 grams of O2(g) reacts with an excess of C5H12(l) and 0.376 moles of CO2(g) is formed, determine the percent yield of CO2(g).

Solved • Dec 10, 2019