20) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H2O2() 2 H20(1) + O2(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure? A)-2.31 x 10 kJ B) -11.5 kJ C) 1.44 kJ D) -0.0217 kJ E) -23.1 kJ ahast in energy?

20) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H2O2() 2 H20(1) + O2(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure? A)-2.31 x 10 kJ B) -11.5 kJ C) 1.44 kJ D) -0.0217 kJ E) -23.1 kJ ahast in energy?

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

A student dissolves 13.2 g of sodium hydroxide (NaOH)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 21.0 °C to 33.4 °C over the course of 5.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: + NaOH (s) — Na" (ад) + ОН (ад) olo You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. Ar Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. exothermic x10 Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ Calculate the…
A 1.27-g sample of fumaric acid (C4H4O4) is burned in a bomb calorimeter and the temperature increases from 24.70 °C to 27.50 °C. The calorimeter contains 1.01×103 g of water and the bomb has a heat capacity of 755 J/°C. Based on this experiment, calculate ΔE for the combustion reaction per mole of fumaric acid burned (kJ/mol).
A chemist measures the energy change AH during the following reaction: 2 HgO(s) → 2 Hg(1)+0,(9) AH=182. kJ Use the information to answer the following questions. endothermic. This reaction is... x10 exothermic. Suppose 61.0 g of HgO react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. |kJ Round your answer to 3 significant digits.
4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
A chemist measures the energy change AH during the following reaction: C;Hg(9)+50,(g) → 3 CO2(9)+4H,0(1) AH=-2220. kJ Use the information to answer the following questions. endothermic. This reaction is... x10 exothermic. Suppose 10.9 g of C,Hg react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits.
4. Two solutions, initially at 24.60°C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J/°C). When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30°C. Determine the AH°rxn for the reaction. Dsol'n = 1.00 g/mL. Csol'n = 4.184 J/g°C.
Calculate the ΔH°rxn of the reaction in a bomb calorimeter: NaOH(s) → NaOH(aq) Given the following: Volume of solution = 100mL (when solid added to water) Concentration = 1M Mass of NaOH = 1.0359g Change in temperature = 2.5°C Specific heat capacity of solution = 4.184 J/°C Specific heat capacity of bomb calorimeter = 30 J/°C Molecular mass of NaOH = 40g/mol
A chemist measures the enthalpy change AH during the following reaction: COCL,(9) + 4 NH,(g)–+cO(NH,),(s) + 2 NH,Cl(s) AH=-559. kJ Use this information to complete the table below. Round each of your answers to the neare reaction AH co(NH,),(-) + NH,CI(3) - coC, () + 2NH, (2) 3coCI, (3) + 12NH, (3) - 3c0(NH,), (-) + 6NH,CI(s) co(NH,),() + 2NH,C1(«) → COCI, (3) + 4NH, (2) Explanation Check MacBook Air 20 F1 F3 F4 F5 F6 F @ & くC
A chemist measures the enthalpy change AH during the following reaction: 2 Al(s) + Fe₂O3(s)→Al₂O3(s) + 2 Fe(s) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction 3A1₂03 (s) + 6Fe(s) Al₂O3(s) + 2Fe(s) AH-852. kJ 6Al(s) + 3Fe₂O3(s) 2Al(s) + Fe₂O₂ (s) Al(s) + Fe₂O₂ (s) → — Al₂O₂ (s) + Fe(s) = ΔΗ kJ kJ ☐ kJ ☐ x10 X
Calculate the change in internal energy (ΔE) for a system that is giving off 3.0 kcal of heat and is changing from 1.00 L to 8.00 L in volume at a pressure of 2.00 atm. (Remember that 101.3 J = 1 L∙atm; 1 cal = 4.18 J)
The thermite reaction is a very exothermic reaction; it has been used to produce liquid iron for welding. A mixture of 2 mol of powdered aluminum metal and 1 mol of iron(III) oxide yields liquid iron and solid aluminum oxide. How many grams of the mixture are needed to produce 219 k) of heat? Data: AH;(Al(s)) = 0 kJ/mol AH (Fe,O3 (s)) = -825.5 kJ/mol AH (Fe(1)) = 12.4 kJ/mol AH;(Al2O3 (s)) = -1675.7 kJ/mol
Consider the combustion of propane: C3H (9) + 50, (9)→ 3CO, (9) + 4H2 O(1) AH = -2221 kJ A balloon is being inflated to its full extent by heating the air inside it. In the final stages of this process, the volume of the balloon changes from 4.00 x 10° L to 4.50 x 10° L by the addition of 1.4 x 10 J energy as heat. Assume that all the heat comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 50.% efficient? Mass =