When in danger, bombardier beetles can fire a hot, toxic mixture of chemicals at theirattacker. This mixture contains quinone, C6H4O2, a compound that is formed by thereaction of hydroquinone, C6H4(OH)2, with hydrogen peroxide, H2O2.The equation for the overall reaction is:→ CHO,CH (OH), + H,O,->2(aq)+ 2H,0,2(aq)2(aq)()mentHCIUse the following data to calculate the enthalpy change, in kJ mol-1, for the above reaction.enAH = + 177.4 kJ mol-g bevloaaibAH = -191-2kJ mol-CH (OH),CHOa4)+ H.2(g)2( aq)2( aq)H,ODios H->2(aq)->20 218)→ H,OAH = -241-8 kJ mol!+ ½0,2(g)H¸O →H,O)AH = -43-8 kJ mol!

Hess's law is defined as the law which states that the total amount of heat absorbed or released for…

When in danger, bombardier beetles can fire a hot, toxic mixture of chemicals at their attacker. This mixture contains quinone, C6H4O2, a compound that is formed by the reaction of hydroquinone, CsH4(OH)2, with hydrogen peroxide, H2O2. The equation for the overall reaction is: CH,(OH),g) + H,O -> 2(aq) CHO + 2H,0 2(aq) 2(aq) Use the following data to calculate the enthalpy change, in kJ mol-1, for the above reaction. CH(OH)g) eno H + CHOag) + H, -> ΔΗ- = + 177-4 kJ mol- 9. 2(g) H,Oaq) AH = -191-2 kJ mol-! -> 2(g) H ½0, AH = -241-8 kJ mol- %3D 2(g) 2(g) (8), H,O → H,O AH = -43-8 kJ mol (g)

When in danger, bombardier beetles can fire a hot, toxic mixture of chemicals at their attacker. This mixture contains quinone, C6H4O2, a compound that is formed by the reaction of hydroquinone, CsH4(OH)2, with hydrogen peroxide, H2O2. The equation for the overall reaction is: CH,(OH),g) + H,O -> 2(aq) CHO + 2H,0 2(aq) 2(aq) Use the following data to calculate the enthalpy change, in kJ mol-1, for the above reaction. CH(OH)g) eno H + CHOag) + H, -> ΔΗ- = + 177-4 kJ mol- 9. 2(g) H,Oaq) AH = -191-2 kJ mol-! -> 2(g) H ½0, AH = -241-8 kJ mol- %3D 2(g) 2(g) (8), H,O → H,O AH = -43-8 kJ mol (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

Commercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)4 (aq) + 3 H2 (g) If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HC1 through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H₂O(1) + CO₂(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.029 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. X Ś
You are carrying out an experiment to determine the MW of a solid acid with the generic formula H3A. You weigh out 0.362 g of the solid acid in a weigh boat and transfer it to a 125 mL Erlenmeyer flask. After dissolving the acid in 25 mL of distilled water, you add 22.51 mL of 0.343 M Sr(OH)2 (aq) solution with a buret until your indicator changes color at the equivalence point. What is the molar mass of the solid acid in units of g/mole? Enter your answer with at least 4 significant digits (Canvas sometimes truncates zeros so assume that all numbers in this question have at least 4 sig figs (ie if Canvas tells you there are 12.3 mL assume 12.30 mL). This question will require precision so don't round any numbers until your final answer.
To measure the amount of calcium carbonate (CaCO3) in a seashell, an analytical chemist crushes a 4.20 g sample of the shell to a fine powder and titrates it to the endpoint with 302. mL of 0.210M hydrogen chloride (HCI) solution. The balanced chemical equation for the reaction is: 2HCl(aq) + CO3(aq) → H₂CO3(aq) + 2Cl¯ (aq) 1 What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of CaCO3 in the sample. Be sure your answer has 3 significant digits. precipitation O acid-base O redox 0 0 0 п% X
In the neutralization of aqueous acetic acid with aqueous calcium hydroxide, 55.7 mL of 0.100 M Ca(OH)2 was required to react with 15.0 mL of CH3COOH. What was the molarity of the acetic acid solution?
How many millilitres of 0.590 mol L−1 H2SO4(aq) are required to completely neutralize 28.1 mL of 0.570 mol L−1 KOH(aq) ? Hint: Write a balanced chemical equation for the reaction. Give your answer in mL, accurate to three significant figures
The substance methylamine is a weak base like ammonia. Write an equation for the reaction that takes place between hydrolodic acid, HI, and methylamine, CH,NH,, when aqueous solutions of the two are mixed. Write the product in ionized form, but the reactants in molecular form. It is not necessary to include states such as (aq) or (g).
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCI through this reaction: HCl(aq) + NaHCO3(aq) NaCl(aq) + H₂O(1) + CO₂(g) The CO₂ gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 200 ml of a 0.050 M HCI solution. What mass of NaHCO, would he need to ingest to neutralize this much HCI? Be sure your answer has the correct number of significant digits. X
A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
In the following chemical reaction, which species is the reducing agent? 2 10, (aq) + 12 H (aq) + 10 Ag(s) + 10 CI (aq)→ 10 ABCI(s) + 1,(s) + 6H,O(1) O Ag O 105 O It is not a redox reaction.
Aspirin, acetylsalicylic acid, C9H8O4, reacts with basic substances. If the titration of an aspirin tablet (with mass equal to 1,000 g) requires 25.43 mL of 0.100 M NaOH to reach the end point. How many grams of acetylsalicylic acid are in the tablet? What is the percent by mass of acetylsalicylic acid in the tablet?
Use the solubility rules to predict whether the following ionic compounds are soluble in water: (a) Na 3PO 4; (b) Mg 3(PO 4) 2; (c) KOH.