Nitroglycerin (C3H;N3O9) is a powerful explosive. Its decomposition may be represented by 4C3H3N309 → 6N, + 12CO, + 10H,O + 02 This reaction generates a large amount of heat and gaseous products. It is the sudden formation of these gases, together with their rapid expansion, that produces the explosion. (a) What is the maximum amount of 0, in grams that can be obtained from 2.00 x 10° g of nitroglycerin? (b) Calculate the percent yield in this reaction if the amount of O2 generated is found to be 6.51 g. %

Nitroglycerin (C3H;N3O9) is a powerful explosive. Its decomposition may be represented by 4C3H3N309 → 6N, + 12CO, + 10H,O + 02 This reaction generates a large amount of heat and gaseous products. It is the sudden formation of these gases, together with their rapid expansion, that produces the explosion. (a) What is the maximum amount of 0, in grams that can be obtained from 2.00 x 10° g of nitroglycerin? (b) Calculate the percent yield in this reaction if the amount of O2 generated is found to be 6.51 g. %

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

Calculate the reacting masses as given in the questions.
If 35g of LiCl mixes with 25g of Ca(OH)2, (a) which is the limiting reactant? (b) what is the theoretical yield? LiCl + Ca(OH)2 → LiOH + CaCl2
Be sure to answer all parts. The balanced equation for the reaction of aluminum metal and chlorine gas is 2Al(s) + 3Cl₂(g) → 2AIC13(s) Assume that 0.42 g Al is mixed with 0.52 g Cl₂. (a) What is the limiting reactant? Cl₂ Al (b) What is the maximum amount of AlCl3, in grams, that can be produced? g AIC13
Nitrogen (N2)and hydrogen (H2) react to form ammonia(NH3). Consider the mixture of N2 and H2 shown in theaccompanying diagram. The blue spheres represent N, andthe white ones represent H. (a) Write the balanced chemicalequation for the reaction. (b) What is the limiting reactant?(c) How many molecules of ammonia can be made, assumingthe reaction goes to completion, based on the diagram?(d) Are any reactant molecules left over, based on the diagram?If so, how many of which type are left over?
If Na3PO4.12H2O was the limiting reactant, and the mass of BaCl2.2H2O was 4.88 gram, the mass of barium phosphate formed would be :( Molar Mass of BaCl2.2H2O = 244g/mol, Molar Mass of Na3PO4.12H2O = 380g/mol, Molar Mass of Ba3 (PO4)2 =602g/mol).
11)
7.) A Sample Of 13.3g of Fe₂03 reacts with 16.89 CO со to yield Fe and Co₂. The balanced equation Fe₂O3 (s) + 3 C0g 2 Fe (5) + 300₂ (g) is Which Substance is the limiting reactant? What is the theoretical yield of Fe ? If the actual experimental yield for Fe is 8.41g what is the percent yield of Fe?
Consider the following unbalanced chemical reaction: Br2 + F2 → BrF5 How many grams of fluorine gas (F2) would be required to completely react with 100.0 grams of bromine (Br2)?
The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.
A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula
[References] TUTOR Chemical Equations: Gram/Gram Calculation Consider the reaction: SOe) + H;O(1) → H3SO;( Given an initial mass of 15.3 g SO, an excess of H50, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H7SO3 produced by the reaction.
The theoritical yeild of a certain compound according to a chemical reaction is 127 g. The percent yield is 82.0%. When the reaction is carried out, what is the actual yeild?