2 1.NaliH, EthanolHgSO,2.1,0H,OPBryKCNI.NAOH, H,Oe.2. H,O1.(CF,CO,)Hg,2. NaBH4(CHs)3P-C(CH3)2THFg.CH2OH1.NaHh.2. CHsBri.AICI,

Answered: I.NallH Ethanol HgSO H,O" 2.1,0 PBr…

I.NallH Ethanol HgSO H,O" 2.1,0 PBr I.NaOH, H,O KCN e. 2. H,О 1.(CF,CO,)Hg. f. 2. NaBH4 (CHs) P-C(CH3)2 THF 9. CH2OH 1.NaH h. 2. C,H3B AICI,

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...

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Using data for DHof (KJ/mol) provided below, calculate DHoRxn for: N2O(g) + 3H2(g) ---> N2H4 (l) + H2O (l) DHof (KJ/mol): N2O(g) = 33.85 ; H2 (g)= 0 ; N2H4 (l)= 50.4 ; H2O(l) = -285.8
Given that H2(g) + F2(g) ---> 2HF(g) Δ?∘rxn=−546.6 kJ⋅mol−1 2H2(g)+O2(g) ⟶ 2H2O(l) ΔHrxn∘=−571.6 kJ⋅mol−1 calculate the value of Δ?∘rxn for 2F2(g)+2H2O(l) ⟶ 4HF(g)+O2(g)
- Consider the problem below: (Equation 1) 2 HF(g) ---> H2(g) + F2(g) ΔH = 537 kJ/mol (Equation 2) C(s) + 2 F2(g) ---> CF4(g) ΔH = -680. kJ/mol (Equation 3) 2 C(s) + 2 H2(g) ---> C2H4(g) ΔH = 52.3 kJ/mol (Equation 4) C2H4(g) + 6 F2(g) ---> 2 CF4(g) + 4 HF(g) ΔH = ??????? To find ΔH for equation 4 you must: Screen Reader Version Consider the problem below: (Equation 1) 2 HF(g) arrow H2(g) + F2(g) ΔH = 537 kJ/mol (Equation 2) C(s) + 2 F2(g) arrow CF4(g) ΔH = minus 680. kJ/mol (Equation 3) 2 C(s) + 2 H2(g) arrow C2H4(g) ΔH = 52.3 kJ/mol (Equation 4) C2H4(g) + 6 F2(g) arrow 2 CF4(g) + 4 HF(g) ΔH = ??????? To find ΔH for equation 4 you must: flip equation 1 only flip equation 2 only flip equation 3 only flip equation 1 and equation 2 only flip equation 1 and equation 3 only flip equation 2 and equation 3 only flip no equation
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the average molecular mass for this sample
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 1.43 g/L at 26 °C and 0.405 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of CH2F2 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111-trifluoroethane (C2H3F3) has a density of 2.39 g/L at 23 °C and 0.593 atm. 1. Calculate the average molecular mass for this sample. 2. Calculate the volume percentage of C2H3F3 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111- trifluoroethane ((C2H3F3) has a density of1.95 g/L at 23 °C and 0.432 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of C2H3F3 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 2.99 g/L at 22 °C and 0.810 atm. Calculate the average molecular mass for this sample.8.94×101 amu Calculate the volume percentage of CH2F2 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the volume percentage of CH2F2 in the sample.
What is the ∆G◦ (in kJ mol−1) for the followingreaction at 25 ◦C?NO2(g) ⇌ N2O4(g)NO2(g):∆H◦ = 33 kJ mol−1; S◦ = 240 J mol−1 K−1N2O4(g):∆H◦ = 11 kJ mol−1; S◦ = 304 J mol−1 K−1A. −41.1 B. −8.8 C. −2.5 D. 16.2E. 5.24 × 104
When nitric acid reacts with hydrazine (i.e. dinitrogen tetrahydride), nitrogen gas and water are formed. The temperature is constant at 25°C.4 HNO3(aq) + 5 N2H4(l) " 7 N2(g) + 12 H2O(l)Substance ΔHf° (kJ/mol) S° (kJ/mol K)HNO3 (aq) –133.9 0.2669H2O (l) –285.8 0.0700N2 (g) 0 0.1916N2H4 (l) +50.6 0.1212a. Calculate ΔH° (in kJ/mol) and ΔS° (in kJ/mol K).b. Calculate ΔG° (in kJ/mol).c. Determine K for this reaction.
C(s) + 2H2(g) CH4(g) ΔH° = –75 kJ exo/endo - thermic Δν(gas) = __, (decrease)Vtot --> which way will equation shift? what will happen if there is an increase in: P(CH4) shift? __ ...two ways to to lose mass(C)? ___________ higher T shift? __