(e) Provide alternative to the following conventional reaction schemes and state the major advantage of your proposed alternative : one environmentally benign HO LOH (i) + H3CCOCH2C00C2H5- conc. H2SO4 0 °C QH CHO ČH3 NaOH (üi) H3C CH3 ELOH/A
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- The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)3. (a) jf 10.0 mjL of H2jSO4 (sp. jr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to 400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SO4 = 98; SO3 = 80 %3Dc) Calculate the standard enthalpy change for the reaction 3C(s) + 4H2 (g) C;H8 (g) Given that C(s) + O2 (g) CO2 (g) AH° = -394 kJmol·' H2 (g) + ½O2 (g) H2O (I) AH° = -286 kJmol C3H8 (g) + 502 (g) 3CO2 (g) + 4H2O (I) AH° = -2220 kJmol·'
- The table below contains some mean bond energy data: Bond C-C 348 H-H N=N Mean bond energy /kJ mol| 436 944 (i) Balance the equation below for the formation of one mole of ammonia, NH3, from its elements. N2 + H2 NH3 AH = -38 kJmol" (ii)Use the data in the table above to calculate the bond energy of N - H bond in NH3 in the reaction given in (1) above. Comment on why the value obtained is referred to as 'mean bond enthalpy (ii) Use the equation below and data from the table to calculate a value for the C=C bond energy in ethene. Bond H-H C-H C-C 348 Mean bond energy /kJ mol 436 418 нн нн С—С + Н Нэнс- с н AH = -136 kJ mol нн н Ethene Ethanevestion 5 The enthalpy of combustion under a pressure of one atmosphere of one mole of methane at 298K is -212.8 kJ. CH4 (g)+202 (g)>CO2(g) +2H2O(1) a. Calculate the average molecular speed of CO, gas at 298 K (C=12, 0=16) b. Calculate the standard enthalpy of formation of the methane at 298K;AH°(methane(g),298K). Given: AHCH2O(); 298K) = -68.33 kJ/mol); AH(CO2 (g); 298K) = -94.25 kJ/mol) Answer: m/s b) ACH4) %3D kJ/mol A Moving to another question will save this response. rch hp no 96 R U P K alt ctriIdeal Gas Law The pressure P, temperature T, and volume V ofan ideal gas are related by PV = nRT, where n is the number ofmoles of the gas and R is the universal gas constant. For the pur-poses of this exercise, let nR = 1; therefore, P = T/V.a. Suppose that the volume is held constant and the temperatureincreases by ∆T = 0.05. What is the approximate change inthe pressure? Does the pressure increase or decrease?b. Suppose that the temperature is held constant and the volumeincreases by ∆V = 0.1. What is the approximate change in thepressure? Does the pressure increase or decrease?c. Suppose that the pressure is held constant and the volume in-creases by ∆V = 0.1. What is the approximate change in thetemperature? Does the temperature increase or decrease?
- Carbon dioxide from the atmosphere "weathers," or dissolves, limestone (CaCO3) by the reaction CACO3(8) + CO2(9) + H2O(1) → Ca²+ (aq) + 2HCO3¯(aq) Obtain AH° for this reaction using the following data: AH;(CaCO3(8)) = –1206.9 kJ/mol AH;(CO2(9)) = -393.5 kJ/mol AH;(H2O(1)) = –285.8 kJ/mol AH;(Ca²+ (ag) -542.8 kJ/mol AH;(HCO3¯(aq)) = -692.0 kJ/mol ΔΗ kJ %3DWhat volume of benzene (C&H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 1.5 x 103 kJ of heat according to the following reaction? %3D = -6278 kJ 2 C6H6(1) + 15 O2(g) – 12 CO2(g) + 6 H2O(g) AH°, rxn 75 mL 37 mL 21 mL 19 mL 42 mLPart A What volume of methanol is formed if 2.92x1011 L of methane at 1.013 bar pressure and 25 °C is oxidized to methanol? The density of CH3OH is 0.791 g mL-¹. Assume that the oxidation of methane to methanol occurs in a 1:1 stoichiometry. Express your answer numerically in litres. View Available Hint(s) VO ΑΣΦ Submit ? Part B L CH3OH Standard heats of formation The standard heats of formation for selected substances are shown here. Substance CH₁ (9) CH3OH (1) CO₂(g) H₂O(1) O₂(g) Af Ho (kJ mol-¹) -74.8 -238.6 -393.5 -285.83 0 Calculate the standard enthalpy changes for the combustion of a mole of methane and the combustion of a mole of methanol. Assume that the combustion reactions occurs at 25°C, so the water produced is liquid. Enter the enthalpy for methane followed by the enthalpy for methanol in kJ mol-¹ separated by a comma to four significant figures.
- Methanol is known to be the simplest alcohol, and is used as an antifreeze agent, a solvent, a fuel anda denaturant for ethyl alcohol. It is also known as “wood spirit”, as it is obtained from the pyrolysis ofwood. Methanol burns in air to produce CO2(g) and H2O(l). The chemical reaction is: 2CH3OH (ℓ)+ 3O2 (g) à 2CO2 (g) + 4H2O (ℓ)Calculate the enthalpy change for the reaction using the standard enthalpies of formation are found onthe chart provided.carbon disuifide ic a foul-smelliag soluent that dissoluer sUltur & other nonpolar substances. It can be made by heating sultur in an atmosphere of Methane, For the reaction (berow,AH , = 760.4 uJ and ASrxn= 1219.1. 3/4. = 1219.1 1/14• 4 CHucgs t Sg C =acs2egs + 8 Hz eg ) Part 1 Calcuiate the equilibrium Consfant ar 250 -o°C. Part 2 Calculate the equilibriun consiant at 500.0°c.1) CH;CO0 (aq) + HC,H-0, (aq)=C,H¿COOH (aq) + C,H,O," (aq) 2) CIO" (aq) + HC,H;O, (aq) C,H,O, (aq) + HCIO (aq) 3) C,H;COOH (aq) + CIO (aq)= HCIO (aq) + C,H5C00 (aq) %3D it Arrange the substances based on their relative acid strength. CIO C,H,0, strongest acid C,HCO0 intermediate acid HCIO weakest acid HC,H,04 not a Bronsted-Lowry acid C,H;COOH