Given the following balanced chemical equation: 2 CO(g) + O2(g) 2CO2(g) 15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction a) Determine the limiting and excess reactant. Calculate the mass of product produced to support your answers. b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield? Percent yield actual yield theoretical yield x 100 c) Calculate the mass of the excess reactant left over.

Given the following balanced chemical equation: 2 CO(g) + O2(g) 2CO2(g) 15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction a) Determine the limiting and excess reactant. Calculate the mass of product produced to support your answers. b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield? Percent yield actual yield theoretical yield x 100 c) Calculate the mass of the excess reactant left over.

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

According to the balanced reaction below, calculate the quantity of moles of NH, gas that form when 4.20 mol of N,H, liquid completely reacts: 3 N,H,(1) → 4 NH,(g) + N,(g)
2 Mg(s) + O2(g) -> 2 MgO(s) When 1.5 g of magnesium burns, the theoretical yield of magnesium oxide is ____ g.
According to the following reaction, how many grams of hydrofluoric acid will be formed upon the complete reaction of 26.4 grams of water with excess silicon tetrafluoride? silicon tetrafluoride (s) + water (I) --> hydrofluoric acid (aq) + silicon dioxide (s) O58.6g O 2.9g O 14.7g 20.2g
How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic
22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?
How many moles of water are produced when 6.33 moles of CH4 react? CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (g) (balanced)
In the reaction below, 7.0 mol of NO and 5.0 mol of O2 are reacted together. The reaction generates 3.0 mol of NO2. What is the percent yield for the reaction? 2NO (g) +O2 (g)2NO2 (g)
What is the percent yield if 28.16 g of CO2 is collected from a reaction with a theoretical yield of 225.3 g of CO2? 20.00% 50.00% O 25.00% O 12.50%
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 gg of Mg are allowed to react with 10.5 g of O2, 13.4 gg of MgO are collected. Determine the limiting reactant for the reaction. Express your answer as a chemical formula.
Use the balanced equation to answer the question follows. 2C2H6(g)+5O2(g) -----> 4CO(g)+6H2O(g) to calculate how many moles of O2 are needed to react completely with 1.6 moles of C2H6?
A Moving to another question will save this response. Question 7 Consider the following balanced reaction. What mass (in g) of C0 2 can be formed from 288 mg of O 2? Assume that there is excess C 3H 7SH present. C3H 7SH( ) + 6 0 2(8) - 3 CO 2( g) + SO 2(g) + 4 H 20( g) O 0.126 g CO2 O 0.396 g CO2 O 0.209 g CO2 O 0.198 g CO2 O 0.792 g CO2 A Moving to another question will save this response.