9.24 For each of the following reactions, 20.0 g of each reactant is A present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced. a. 4Al(s) + 302(g) b. 3NO2(g) + H2O(l) 2Al2O3(s) (Al2O3) →2HNO3(aq) + NO(g) (HNO3) c. C₂H₂O(l) + 302(g) 2CO2(g) + 3H2O(g) (H₂O) A

9.24 For each of the following reactions, 20.0 g of each reactant is A present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced. a. 4Al(s) + 302(g) b. 3NO2(g) + H2O(l) 2Al2O3(s) (Al2O3) →2HNO3(aq) + NO(g) (HNO3) c. C₂H₂O(l) + 302(g) 2CO2(g) + 3H2O(g) (H₂O) A

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.100QE

See similar textbooks

Similar questions

2N2(g) + 3O2(g) ® 2N2O3(g) DH°rxn = +86.6 kJ 1. When 12.0 moles of N2 react, the reaction heat is ____________ kJ 2. To make +552 kJ of reaction heat, _________ moles of O2 must react. 3. To make +24 kJ of reaction heat, a count of ________________ N2O3 molecules must form.
An Iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal. __Fe2O3(s)+__CO(g)-->__Fe(s)+__CO2(g) a) balance this equation b) Calculate the grams of CO that can react with .350kg of Fe2O3 c) Calculate the grams of Fe and the grams of CO2 formed when .350kg of Fe2O3 reacts
The manufacture of aluminum includes the production of cryolite (Na3AlF6) from the following reaction: 6〖HF〗_((g))+3〖NaAlO〗_(2(s))→ 〖Na〗_3 〖AlF〗_(6(s))+3H_2 O_((l))+ 〖Al〗_2 O_(3(s)) How much HF (hydrogen sulfide) is required to produce 2.50kg of Na3AlF6? How many cm3 of HF(g) are needed to produce 26.0g of Na3AlF6? The density of HF (g) at 25is 1.15g/L.
for each of the following reactions, 20.0g of each reactant is present initially. determine the limiting reactant, and calculate the grams of product in parentheses that would be produced a. 4Al + 3o2 -> 2Al2o3 (Al2O3)
Glucose oxidation is a chemical process that provided energy for an organism to carry out all of its regular activities. The equation for the oxidation of glucose (C6H12O6) is: C6H12O6(aq) + 6O2(aq) →6CO2(aq) + 6H2O(ℓ) How many moles of O2 are needed to completely react with 31.94 g of C6H12O6 ? Answer to 2 decimal places.
In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide and water. 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(g) (a) How many moles of O2 are needed to react with 6.00 moles of C2H2?(b) How many moles of CO2 are produced when 4.5 moles of C2H2 reacts?(d) How many moles of CO2 are produced from 0.100 mole O2?
Given the following reaction. 2Na2S + __Na2CO3 + __SO2(g) __Na2S2O3 + CO2(g) DH =-1025kJ A. Balance the above equation by filling in the missing coefficients. B. Provide the name of Na2CO3. C. How many grams of CO2(g) would be produced if 12.5g SO2(g) reacted with 10.0g Na2S. Assume Na2CO3 is in excess.
Methane, CH4, reacts with oxygen to produce carbon dioxide, water, and heat. CH4(g) + 2O2(g)  CO2(g) + 2H2O(l) ΔH = – 890.3 kJ What is the value of ΔH if 5.00 g of CH 4 is combusted?
Hydrogen gas reacts with chlorine gas to produce hydrogen chlorine gas The hydrogen chloride gas can be easily dissolved in water to form hydrochloric acid. HOW MANY MOLES OF HYDROGEN ARE PRODUCED BY THE DECOMPOSITION 1.000 * 10^3grams of water?
Consider the gaseous reaction at N2+3H 2 2NH 3 2.00 mole of N2 and 3.00 mole of react , H_{3} which of the two reactants is the limiting reactant ?
In the acetylene torch, acetylene gas (C2H2)(C2H2) burns in oxygen to produce carbon dioxide, water, and energy: How many moles of O2O2 are needed to react with 3.00 molmol of C2H2C2H2? How many moles of CO2CO2 are produced when 4.8 molmol of C2H2C2H2 react? How many moles of C2H2C2H2 are required to produce 0.70 molmol of H2OH2O? How many moles of CO2CO2 are produced when 0.180 molmol of O2O2 reacts?
Aqueous sulfuric acid H2SO4 reacts with solid sodium hydroxide NaOH to produce aqueous sodium sulfate Na2SO4 and liquid water H2O. If 18.8g of sodium sulfate is produced from the reaction of 33.3g of sulfuric acid and 39.4g of sodium hydroxide, calculate the percent yield of sodium sulfate.