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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:One reason for learning about the factors that affect spontaneity is that we can use
this knowledge in the lab to manipulate reaction conditions in order to favour the
production of reactants to product(s) of interest. Which of the following statements
accurately describe strategies that are available to a chemist to manipulate the
outcome of a reaction?
The product can always be favoured by adding heat to the reaction, to drive the
equilibrium towards products.
If the product is not favoured under standard conditions, there is nothing that
can be done to favour the products other than try to produce it a different way
(i.e., by using a different reaction).
If the product is not favoured under standard conditions, it may be possible to
adjust the concentrations of reagents and products in order to favour the
forward reaction.
If the reaction is enthalpically favoured but entropically opposed, the product
may be favoured by lowering the temperature.
If the product is not favoured at first, just leave it stirring longer and eventually
all of the reactants will be converted to products.
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- Gaseous octane (C8H18) is burned with dry air in a combustor to produce an equilibrium mixture of H2O(g), CO2, O2, N2, H2, OH, CO, and NO at 1400 K and 20 atm. Calculate the equilibrium composition (number of moles or mole fractions) for fuel-air equivalence ratios of 0.6 and 1.4.arrow_forwardGive detailed Solution...don't give Handwritten answerarrow_forwardThe equilibrium constant for the reaction 2 C3H6(g) ↔ C2H4(g) + C4H8(g) Is found to fit the expression: lnK = A + B/T + C/T2, between 300 and 600 K, where A = -1.04, B = -1088 K, C = 1.51x105 K2. Calculate the standard reaction enthalpy and standard reaction entropy at 400 Karrow_forward
- Consider the vaporization of carbon disulfide. CS₂ (1) = CS₂(g) Free energies and enthalpies of formation can be found here Calculate the standard free energy for this reaction and the standard enthalpy for this reaction. AG = K25C 2.5 Calculate the equilibrium constants for this reaction at 25 °C and at CS₂'s normal boiling point. Tbp 0.346 Incorrect Calculate the normal boiling point of CS₂. 290.322 kJ/mol Incorrect ΔΗ° = 27.7 °C Kbp 0.355 Incorrect kJ/molarrow_forwardCarbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constant for this reaction using the AG; values in the table. Substance AG; (kJ/mol) H,CO, (aq) -616.1 H,O(1) -237.1 CO,(g) -394.4 K = Carbonic acid then ionizes in water (K = 4.5 x 10-7). Ignoring K2, estimate K for the overall process by which CO, and H,O form H* and HCO,. K = What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Роо, atmarrow_forwardFor the reaction A(aq) ---> B(aq) the variation in the standard free enthalpy is 3.50 kJ at 25 oC and 4.64 kJ at 45 oC. Calculate the value of the equilibrium constant for this reaction at 75°C.arrow_forward
- Use the References to access important values if needed for this question. For the reaction NH,Cl(aq)- NH3(g) + HCI(aq) AG° = 64.7 kJ and AH° =86.4 kJ at 274 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 274 K. The entropy change for the reaction of 2.44 moles of NH,Cl(aq) at this temperature would be J/K. Submit Answer Retry Entire Group 4 more group attempts remaining edarrow_forwardFor the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 22.7 at 25oC and 37.3 at 50oC. What is the value of the change in the Gibbs standard free enthalpy (in kJ) of this reaction at 75oC?arrow_forward
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