at aChoose...Choose...exothermicinverselyendothermicdirectlyChoose...Choose...s at The following reaction is :CH,OH ) + 3/2 0,+ CO.2H,0+ 726.4 kJ+(1)2(9)Choose...

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The following reaction is : CH,OH ) + 3/2 0, + CO. 2H,O) + 726.4 kJ + (1) 2(9) Choose...

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 23QAP: In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The...

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In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g)+4H2(g)NH3(g)+3H2O(g)H=637kJ (a) Calculate H when one mole of hydrogen gas reacts. (b) What is H when 10.00 g of NH3(g) are made to react with an excess of steam to form HN3(g) and H2 gases?
The emission of NO, by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction: 2 CO(NH;)»(3) + 4 NO(3) + O2(8) 4 Na(8) + 2 CO;(g) + 4 H¿O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 Kand contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react complete- ly with the NO formed during 8.0 hours of driving?
For all of the following experiments, under standard conditions, which species could be spontaneously produced? (a) A lead wire is placed in a solution containing Cu2+ No reaction. YES or NO Cu. YES or NO PbO2. YES or NO (b) Crystals of I2 are added to a solution of NaCl. No reaction. YES or NO I^-. YES or NO Na. YES or NO (c) Cl2 gas is bubbled into a solution of NaI. Cl^-. YES or NO No reaction. YES or NO Na. YES or NO
9-4. For each of the following reactions: (1) Calculate the enthalpy change for the reaction using Standard Enthalpy of Formation values from the table posted on the Course Resources page. (2) State whether the reaction is endothermic or exothermic. а. 3 Са0() + 2 Feе(s) > Fe,0%3(s) +3 Сa('s) b. 2 C;Ho(g) + 7 02(g) → 4 CO2(g) + 6 H2O()
5. Reaction Enthalpy. and calculate AH for the following chemical equations. AH (kJ/mol): HCN = 130.5, Cas(PO4)2=-4120.8, H3PO4--1288, SiCl=-640.1, SiO₂= -910.9, Mg0=-601.6, HCl--167.16 b) Ca₂(PO4)2(s) + H₂SO4(0)- 0 CaSO4(s) + H3PO4(1)
5. Reaction Enthalpy. balance and calculate AHa for the following chemical equations. AH (kJ/mol): HCN = 130.5, Cas(PO4)2=-4120.8, H3PO4--1288, SiCl₁=-640.1, SiO₂= -910.9, Mg0=-601.6, HCl=-167.16 c) SICIL(1)+H₂O() SIO₂ (s) + нск HCl(aq)
Write the balanced net ionic equation for the reaction of aqueous sodium sulfate with aqueous lead(II) nitrate. Include phases. net ionic equation: Pb2+ (aq) + S²- (aq) PbS(s) Incorrect SPECIAL ΔΣΩ λμπ x"| Xo EX| (s) (1) || (aq) (g) () [] CLR
Use the standard reaction energies given below to determine AG*rxn for the following reaction: XY4(g) + Y₂O(g) --> XO(g) + 3Y2(g) Given: 2Y2(g) + XO(g) --> XY3OY(1) 2XY4(g) + O2(g) --> 2XY3OY(1) 2Y2(g) + O2(g) --> 2Y2O(g) Give answer in KJ/mol. Give answer to two decimal places. Do not include units answer. DG = -155.61 kJxmol-1 DG = -139.48 kJxmol-1 DH° -147.08 kJxmol-1
The standard reaction enthalpy for 2 CO(g) ---> 2 C(s) + O2(g) is: +2 ΔHf°[CO(g)] + Δ>Hf°[CO(g)] - ΔHf°[CO(g)] -2 Δ>Hf°[CO(g)] +2 ΔHf°[C(s)] + ΔHf°[O2(g)]
The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application todaY, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H, SO,() – SO;(9) + H,O() AH-+113. kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) – PbO,(s) - 2 S0, (g) → 2 PbSO,(s) AH= -775. J Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ.
8. (I1.7) Using the following reactions at 298 K: CH,CHO + 2 H + 2e + CH;CH;OH E = -0.197 V NAD + H + 2e + NADH E = - 0.320 V Calculate the equilibrium constant for the first step in the metabolism of ethanol (CH,CH,OH) given by the following reaction: CH,CH,OH + NAD' + CH,нО + NADH + H' 9. (II.8) The dissociation constant (K) of a 0.010 M solution of a monoprotic acid at 298 K is 1,47 x 10$. Calculate the percent dissociation (%) by using a mean activity coefficient Y = 0.93. HA H + A
1- Using the information in the table below, calculate the heat of released from the following reaction in kJ per g of NO. ( Mw. Of NO = 30.01 g/mol). %D + 502 (g) 6H,0(9) + 4 NO, (6), 4NH, '3(g) NH, H,0 NO H,° (kJ/mol) - 46.1 |-241.8 + 90.3 Select one: а.-5.678 b. -13.29 С. -8.372 d. -7.541 е. -30.16