The 12 key principles of Green Chemistry were formulated by P.T. Anastas and J.C. Warner in 1998. It outlines an early conception of what would make a greener chemical, process, or product. Based on your understanding of the 12 Principles of Green Chemistry, choose which principle(s) aim at reducing: (i). materials (ii). waste

The 12 key principles of Green Chemistry were formulated by P.T. Anastas and J.C. Warner in 1998. It outlines an early conception of what would make a greener chemical, process, or product. Based on your understanding of the 12 Principles of Green Chemistry, choose which principle(s) aim at reducing: (i). materials (ii). waste

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

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The enthalpy change for the reaction C(s, graphite) + 1⁄2O2(g) --> CO(g) cannot be measured directly since some carbon dioxide is always formed in the reaction. It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide. C(s, graphite) + O2(g) --> CO2 ΔH=-394 kJmol–1 CO(g) + 1⁄2O2(g) --> CO2 ΔH=-283 kJmol–1 The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is
Green Chemistry and Atom Economy The purposeful design of chemical products and processes that minimize the use of environmentally hazardous substances and the generation of waste is known as green chemistry. Green chemistry is a philosophical approach that is being applied to many areas of science and technology, and its practice is summarized by guidelines known as the “Twelve Principles of Green Chemistry” (see details at this website (http://openstaxcollege.org/l/16greenchem) ). One of the 12 principles is aimed specifically at maximizing the efficiency of processes for synthesizing chemical products. The atom economy of a process is a measureof this efficiency, defined as the percentage by mass of the final product of a synthesis relative to the masses of all the reactants used: atom economy = mass of product/mass of reactants × 100%Though the definition of atom economy at first glance appears very similar to that for percent yield, be aware that this property represents a…
Green Chemistry and Atom Economy The purposeful design of chemical products and processes that minimize the use of environmentally hazardous substances and the generation of waste is known as green chemistry. Green chemistry is a philosophical approach that is being applied to many areas of science and technology, and its practice is summarized by guidelines known as the “Twelve Principles of Green Chemistry” (see details at this website (http://openstaxcollege.org/l/16greenchem) ). One of the 12 principles is aimed specifically at maximizing the efficiency of processes for synthesizing chemical products. The atom economy of a process is a measureof this efficiency, defined as the percentage by mass of the final product of a synthesis relative to the masses of all the reactants used: atom economy = mass of product/mass of reactants × 100%Though the definition of atom economy at first glance appears very similar to that for percent yield, be aware that this property represents a…
The enthalpy of reaction for the combustion of C to CO2 is -393.5 kJ/mol C, and the enthalpy for the combustion of CO to CO2 is -283.0 kJ/mol CO:(1) C(s) + O2(g) -----> CO2(g) ΔH = -393.5 kJ(2) CO(g) + 1/2O2(g) -------> CO2(g) ΔH = -283.0 kJUsing these data, calculate the enthalpy for the combustion of C to CO:(3) C(s) + 1/2 O2(g) ------> CO(g) ΔH = ?
A coffee cup calorimeter with a heat capacity of 4.90 J/∘C was used to measure the change in enthalpy of a precipitation reaction. A 50.0 mL solution of 0.360 M AgNO3 was mixed with 50.0 mL of 0.480 M KCl. After mixing, the temperature was observed to increase by 2.80∘C.Calculate the enthalpy of reaction, Δ?rxn, per mole of precipitate formed (AgCl). Assume the specific heat of the product solution is 4.17 J / (g⋅∘C) and that the density of both the reactant solutions is 1.00 g/mL. Calculate the theoretical moles of precipitate formed from AgNO3 and KCl. Calculate the heat change experienced by the calorimeter contents, ?contents. Calculate the heat change experienced by the calorimeter, ?cal. Calculate the heat change produced by the solution process, ?solution. Calulate Δ?solution for one mole of precipitate formed. I'm just going to go ahead and say thank you to whoever decides to answer this question. I really appreciate the help I have received. ?
The standard enthalpy change for the reaction of between sodium hydroxide and hydrochloric acid can be determined experimentally. What is the name given to the enthalpy change in this type of reaction? In one such experiment, 25cm3 each of solutions of sodium hydroxide and hydrochloric acid of concentration 1 mol/dm were mixed. The temperature rose from 270C to 340C. Calculate the standard enthalpy change for the reaction in KJ/mol. (Assume that the specific heat capacity of the solutions is 4.2KJkg-1K-1 and no heat is lost to the calorimeter)
To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.
In a coffee cup calorimeter, a student places 0.500 g of calcium, followed by addition of 50.0 mL of 1.00 M hydrochloric acid. After the reaction took place, a temperature change of 24.7oC was observed. If the reaction solution has the same properties of water and the calorimeter constant is 5.10 J oC-1, what is the enthalpy of reaction in kJ mol-1? (Note: The mass of solution is the mass of all components added.)
The molar enthalpy change for the neutralization reaction: HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l) is ΔrH° = -57.3 kJ/mol. Imagine you mix 60.7 mL of 1.00 M HCl with 75.9 mL of 1.00 M NaOH in a beaker at 24.1 °C. Calculate the final temperature of the solution after the reaction has gone to completion. You will need to assume no heat is lost to the environment, the density of the reaction solution is the same as water, 1.00 g/mL, and the specific heat capacity of the reaction solution is the same as of water, 4.184 J/g°C. Final temperature (°C)?
What is the enthalpy of reaction,change in heat, for the formation of tungsten carbide,WC,from its elements? W(s)+C(graphite) producing WC(s) The enthalpy change for this reaction is difficult to measure directly,because the reaction occurs at a very high temperature.However , the reaction enthalpies of the following reactions are known: 2W(s)+3O(g) producing 2WO3(s);change in heat=-1685,8 kJ C(graphite)+O2(g) producing CO2(g); change in heat =-393,5 KJ 2WC (s)+5O2(g) producing 2WO3(s) +2CO2(g) ; change in heat = -2391,8 KJ
The first and second ionization enthalpies of calcium.Ca, are 596 kJ mol-1 and 1145 kJ mol-1 respectively at 25 °c.Calculate the standard enthalpy change for the processCa(g) → Ca2+(g) + 2e- (g) at this temperature.
Express the reaction enthalpy for the reaction: A + B + C ----> 1/2D + 1/2E + 1/2F in terms of the reaction enthalpies, delta1 H, delta2 H, and delta3 H for the following: B + 2C ---> D + E