Concept explainers
(a)
Interpretation:
The final reactor pressure should be calculated.
Concept introduction:
The
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(b)
Interpretation:
The percentage conversion of propylene when P = 35.1 atm should be explained.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
(c)
Interpretation:
A graph of pressure versus fractional conversion of propylene should be drawn.
Concept introduction:
The Ideal Gas Law is defined as,
Where, the volume (V) occupied by ‘n’ moles of any gas has a pressure (P) at temperature (T) in Kelvin and ‘R’ = Gas constant
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EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- You did an experiment in which you found that 59.8 J was required to raise the temperature of 25.0 g of ethylene glycol (a compound used as antifreeze in automobile engines) by 1.00 K. Calculate the specific heat capacity of ethylene glycol from these data.arrow_forwardThe quantity of 83.0 g of potassium iodide (KI) is added to water to give a solution with a mass of 150. g. Assume that this solution is very dilute and thus has the same heat capacity as water. The dissolution reaction and the associated heat for potassium iodide is KI (s) -→ K+(aq) + I-(aq) qrx = DHrx = +20.3 kJ. Calculate the change in the temperature of the solution.arrow_forwardA solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g•°C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.arrow_forward
- 3.79 g of a gas (66.3 g mol-1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 64.2 J K-1. Prior to mixing everything was equilibrated to 37.3 °C. The resulting solution with a mass of 81.9 g was observed to be at a temperature of 19.9 °C and have a specific heat capacity of 4.57 Jg-1 K-1. Determine q per mole for this dissolution process. Oa. 1.33 x 105 J/mol Ob. -7630 J/mol Oc. 1.96 x 106 J/mol Od. -1.71 x 106 J/mol Oe. 1.71 x 106 J/molarrow_forwardTwo solutions, 100.0 mL of 1.00 M AgNO3 (aq) and 100.0 mL of 1.00 M NaCl (aq), both initially at 22.4oC, are added to a Styrofoam-cup calorimeter and allowed to react. After the reactants are mixed by stirring, the temperature is observed to increase to 30.2oC. The net ionic equation for this reaction isAg+ (aq) + Cl-(aq) → AgCl (s)a) Determine qrxn per mole of AgCl (s) in the reaction.b) Is the reaction endothermic or exothermic?arrow_forwardA student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔH soln. Was the dissolution of this salt exothermic or endothermic?arrow_forward
- The following reaction: 2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l)was studied in a coffee cup calorimeter. In the experiment, 100. mL portions each of 1.00 M aqueous NaOH and H2SO4, each at 24.0°C were mixed. The maximum temperature achieved was 30.6°C. Neglect the heat capacity of the cup and the thermometer, and assume the solution of products has a density of 1.00 g/mL and a specific heat capacity of 4.18 J/g K.What is the heat of reaction, (Delta)Hrxn, for the reaction as written in kJ?arrow_forwardIdentify the effect of the condition on the indicated parameter. Write increase, decrease, or no effect , and provide an explanation The actual concentration of the sodium hydroxide used in the calibration part of the experiment was lower than the stated value. However, the NaOH solution used in the determination of ΔHrxn was of the correct concentration. [magnitude of ΔHrxn]arrow_forwardA student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or 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. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.arrow_forward
- The specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?arrow_forwardA student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = Jarrow_forwardA 104.2 mL sample of 1.00 M NaOH is mixed with 52.1 ml of 1.00 MH2SO, in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 23.05°C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.90 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g°C), and that no heat is lost to the surroundings. 1st attempt Part 11 E See Periodic Table Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation. He (ag).arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning