Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: 2NH; (g) → N,H, (3) +H, (g) Round your answer to zero decimal places.
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- A chemical reaction transfers 30.8 kJ to a thermal reservoir that has a temperature of 45.3 C before and after the energy transfer. Calculate the entropy change for the thermal reservoir.Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: →+Al2O3s3H2g+2Als3H2Og Round your answer to zero decimal places. H2 0 , 0, 130A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 16.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate A G for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
- Use the database on the textbook to calculate the entropy change of the following reaction under standard condition 1bar and 298 K: 2C2H6 (g) + 7O2 (g) = 4CO2 (g)+ 6H2O (L) ΔreactionS = _________ J/K/ (mol reaction). 4 sig. fig. per mole of reaction, not per mole of any subject. The data is copied from the appendix here material standard entropy ( J/K/mol) C2H6 229.60 O2 205.138 CO2 213.74 H2O(L) 69.91Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50 g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40 g of ethylbenzene (PhEt) and 50 g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead you mix 40 g of benzyl alcohol (PhMeOH) into 50 g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as:ΔΔG = ΔmixG[ PhMeOH ∶ PhH ] − ΔmixG[ PhEt ∶ PhH ]What do you expect the sign of ΔΔG to be? ( ΔΔG < 0, ΔΔG ≈ 0, or ΔΔG > 0 )Briefly justify your answer.Consider the reaction:2C2H6(g) + 7O2(g)4CO2(g) ---------> 6H2O(g)Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.69 moles of C2H6(g) react at standard conditions. S°system = _______ J/K
- A 1 mol quantity of hydrogen gas sample was heated at constant pressure from a temperature of 300 K to 500 K. With the entropy transformation process as a function of temperature variation, the heat capacity equation at constant pressure was estimated , Cp = 6.9469 - 0.199 x 10-3 T + 4.808 x 10-7 T2 (J K-1mol-1). Determine the entropy change of the process.Solid iodine, I2(s), has an enthalpy of sublimation ΔHsubl = 62.4 kJ mol-1. Suppose 5.36 g of iodine at a constant temperature of 35.0 oC is allowed to sublime into the atmosphere at a temperature of 50.8 oC. 1.Calculate the entropy change of the system (i.e. the iodine) in J K-1. Enter your answer into the first answer field in accordance with the question statementBenzene (C6H6) has a melting point of 5.50C and an enthalpy of fusion of 10.04kJmol-1 at 25.00C. The molar heat capacities at constant pressure for solid and liquid benzene are 100.4JK-1mol-1 and 133.0JK-1mol-1, respectively. Calculate the change of entropy of system and change of entropy of the surrounding at 100C for the reaction of C6H6(l)---->C6H6(s)
- A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 150.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40g of ethylbenzene (PhEt) and 50g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead, you mix 40g of benzyl alcohol (PhMeOH) into 50g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as: ΔΔG = ΔmixG [PhMeOH ∶ PhH] − ΔmixG [PhEt ∶ PhH] What do you expect the sign of ΔΔG to be? (ΔΔG<0, ΔΔG≈0, or ΔΔG>0)Briefly justify your answer.Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: Fe2O3(s) + 3H2 (g) → +2Fe(s)3 H2O (l) Round your answer to zero decimal places.