5. (10 pts) Sulfuric acid (H2SO4) reacts with sodium hydroxide (NaOH) to produce water (H2O) and sodium sulfate (Na2SO4). In order to react 100 g of sulfuric acid, how many grams of sodium hydroxide are required?

5. (10 pts) Sulfuric acid (H2SO4) reacts with sodium hydroxide (NaOH) to produce water (H2O) and sodium sulfate (Na2SO4). In order to react 100 g of sulfuric acid, how many grams of sodium hydroxide are required?

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter4: Chemical Reactions

Section: Chapter Questions

Problem 4.64P: 4-64 Aspirin is made by the reaction of salicylic acid with acetic anhydride. How many grams of...

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A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
4-64 Aspirin is made by the reaction of salicylic acid with acetic anhydride. How many grams of aspirin are produced if 85.0 g of salicylic acid is treated with excess acetic anhydride?
4-90 Lead(lI) nitrate and aluminum chloride react according to the following equation: In an experiment, 8.00 g of lead nitrate reacted with 2.67 g of aluminum chloride to give 5.55 g of lead chloride. (a) Which reactant was the limiting reagent? (b) What was the percent yield?
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH3 (8) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH3 (g) + 20₂(g) - HNO3(g) + H₂O(g) Suppose the yield of the first step is 81.% and the yield of the second step is 88.%. Calculate the mass of hydrogen required to make 3.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. 0 x10 00 X
Camels store the fat tristearin (C57H110O6) in their hump. As well as being a source of energy, the fat is a source of water, because of the following respiration reaction: 2 C57H110O6 (s) + 163 O2 (g) à 114 CO2 (g) + 110 H2O (l)What mass (g) of water can be made from 1.0 kg of fat?
Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.CCl4(g) + 1/2O2(g) COCl2(g) + Cl2(g), Kc = 4.4 × 109 at 1,000 KCalculate Kc for the reaction 2CCl4(g) + O2(g) 2COCl2(g) + 2Cl2(g). Round off the answer to two significant digits. Group of answer choices 4.4 × 109 8.8 × 109 1.9 × 1010 1.9 × 1019 2.3 × 10–10
The Oxidation of glucose (C6H₁2O6) to carbon dioxide (CO₂) and water, If 968 g of (CH12O6) is consumed,(a): balance the reaction equation.(b) What is the mass of CO₂ produced ? C6H12O6 +0₂ → CO₂+H₂O (10 Marks) C-12 g/mol, H= 1g/mol, O=16g/mol.
A process for synthesizing dichlorodifluoromethane (CCI₂F2), a compound once widely used as a refrigerant, is based on the chemical reactions below. The numbers below each compound are the molar masses in g mol-¹. (1) $ 4 (2) R F CH4 16.04 CC14 153.82 SEP 30 % AE = Number % 5 T + G + What is the percent atom economy (% AE) for the synthesis of CCl₂F₂? Enter an answer accurate to three (3) significant figures. M 6 C 4 Cl₂ 70.91 2 HF ► 20.01 Y MacBook Pro H & 7 ↑ ↑ tvill N U * 00 Submit Assignment 8 J 1 面 CC14 153.82 | CC1₂F2 120.91 M ZA ( 9 K Quit & Save + + O - O W 4 HCI 36.46 L 2 HCI 36.46 Back X P Question Menu A ^ 0 + 11 [ O Next ? } |
5. The reaction of gaseous potassium superoxide, KO, is used in life-support systems to replace CO:(g) in expired air with O:(g). The unbalanoced chemical equation for the reaction is given below. KO:(s) + CO:(g) – K:CO:(s) + O:(g) How many moles of K:CO:(s) are produced per milligram of KO2(s) consumed?
help with both of the same equations
Propylene is burned with oxygen gas to form carbon dioxide and water vapor. If 30 kg of propylene is reacted, how much oxygen gas in kg is needed? Reaction: C3H6(g) + O2(g) = CO2(g) + H2O(g)

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