Jessica is doing her pre-lab homework for Chemistry. She is asked to predict how many grams of oxygen gas are produced if 40.0 g of potassium chlorate isdecomposed according to this balanced chemical equation shown.2KCIO3(s) – 2KCI(s)+302(g)She performs the following calculation, and gets 15.7 g of O2 as her answer.EKCIO,mol KCIO,mol O,80,1 mol KC1O,122.55 g KC1033 mol 0232.00 g 021 mol 022 mol KC1O3The next day when her group performs the experiment they obtain an actual yield of 14.9 grams of oxygen gas. What is the percent yield for the experiment?report your answer to the tenths place, i.e. one decimal place."

Percent yield is the ratio of actual yield to the theoritical yield.

Jessica is doing her pre-lab homework for Chemistry. She is asked to predict how many grams of oxygen gas are produced if 40.0 g of potassium chlorate is decomposed according to this balanced chemical equation shown. 2KCIO3(s) – 2KCI(s)+302(g) She performs the following calculation, and gets 15.7 g of O2 as her answer. Kcio, mol KCIO, mol o, 1 mol KClo, 122.55 g KClo, 3 mol 0, 2 mol KClo, 32.00 g 02 1 mol 0, The next day when her group performs the experiment they obtain an actual yield of 14.9 grams of oxygen gas. What is the percent yield for the experiment? report your answer to the tenths place, i.e. one decimal place.

Jessica is doing her pre-lab homework for Chemistry. She is asked to predict how many grams of oxygen gas are produced if 40.0 g of potassium chlorate is decomposed according to this balanced chemical equation shown. 2KCIO3(s) – 2KCI(s)+302(g) She performs the following calculation, and gets 15.7 g of O2 as her answer. Kcio, mol KCIO, mol o, 1 mol KClo, 122.55 g KClo, 3 mol 0, 2 mol KClo, 32.00 g 02 1 mol 0, The next day when her group performs the experiment they obtain an actual yield of 14.9 grams of oxygen gas. What is the percent yield for the experiment? report your answer to the tenths place, i.e. one decimal place.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Balance chemical equation given below. HoW much lithium nitride is produced when 20 g of lithium and 5 g of nitrogen combine to form lithium nitride, a component of advanced batteries? When the reaction is balanced with the least integers, what is the sum of the coefficients? (Hint: don't forget to add coefficient 1 if it is any.) Li + N2 → LizN (Hint: find a limiting reagent.) MM Li = 6.94 g/mol MM N2 = 28 g/mol MM LigN = 34.83 g/mol %3D Answer: mass(g) =
Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H2 react with 3 moles 02, enter "3" for each, not "1". According to the following reaction: 2Na (s) + 2H20 (I) –→ 2NaOH (aq) + H2 (g) What would you multiply "moles of sodium" by to convert to the units "moles of hydrogen" ? (number) (unit) = moles H2 moles Na (number) (unit)
Consider the unbalanced equation for the combustion of hexane: αC6H14(g)+βO2(g)→γCO2(g)+δH2O(g) Determine how many moles of O2 are required to react completely with 7.4 mol of C6H14. Express your answer using two significant figures.
Be sure to answer all parts. The reaction between aluminum and iron(II) oxide can generate temperatures approaching 3000°C and is used in welding metals: 2AI + Fe,O3 - AhO, +2Fe In one process, 118 g ofAl are reacted with 601 g of Fe,O. Calculate the mass (in grams) of Al,O, formed, and determine the amount of excess reagent left at the end of the reaction. mass of Al,O, formed: amount of excess reagent left:
The reaction between aluminum and iron(III) oxide (known as the thermite reaction) can generate temperatures approaching 3000 °C, and is used in welding metals: Al (s) + Fe2O3 (s) --> Al2O3 (s) + Fe (s) In one particular reaction, 124 g of Al are reacted with 601 g of Fe2O3. Calculate the mass (in grams) of Al2O3 that would be formed.
For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant.C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) 0.0500 molO2 to mol CO2 Express your answer using three significant figures.
be sure your answer is correct and have the correct number of significant digits
Jessica is doing her pre-lab homework for Chemistry. She is asked to predict how many grams of oxygen gas are produced if 40.0g of potassium chlorate is decompose according to this balanced chemical equation shown. 2KCIO3(s)-2KCI(s)+302(g) She performs the following calculation, and gets 15.7 g of O2 as her answer. g KCIO mol KCIO, mol O, 80, 1 mol KC1O3 122.55 g KC1O3 3 mol 02 32.00 g 02 1 mol 0, 2 mol KC1O, The next day when her group performs the experiment they obtain an actual yield of 15.2 grams of oxygen gas. What is the percent yield for the experiment? report your answer to the tenths place, i.e. one decimal place.
c38(g)+5o2(g)=3co2(g)+4h2o(g) how many moles of carbon dioxide would be produced from 20.45 moles of oxygen gas
This is the chemical formula for nickel tetracarbonyl (a powerfully poisonous liquid used in nickel refining): Ni(CO)4 A chemical engineer has determined by measurements that there are 4.98 moles of nickel in a sample of nickel tetracarbonyl. How many moles of carbon are in the sample? Round your answer to 3 significant digits. | mol x10 券

Use the balanced equation, 4K + O2-->2K2O , to answer the following question. How many grams of O2 are needed to react completely with 16.6 g of K ? Be sure your answer has the correct number of significant figures.
fill in blanks and solve using the emthod shown! please