Indicate whether ?G increases, decreases, or does not change when the partial pressure of H2 is increased in each of th...
. Calculate the partial pressure of H2(g) at equilibrium for the following reaction at 90.0°C if the partial pressure of C2H2(g) is 1.8 atm and the partial pressure of C2H6(g) is 0.30 atm. C2H2(g) + 2H2(g) ⇄ C2H6(g) KP = 0.045
Indicate whether the entropy of the system increases or decreases for each of the following processes. Include a BRIEF explanation. Make up a process for (d) and indicate if the entropy of the system increases or decreases in that process, and provide a brief explanation as well. a) Water boiling at 100.0°C b) 2H2(g) + O2(g) ---> 2H2O(g) c) liquid water freezes at 0.0°C d) e) water vapor expanding from 1.0L of volume to 2.0L of volume f) mixing 10mL...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N2(g)+3H2(g)↽−−⇀2NH3(g) the standard change in Gibbs free energy is Δ?∘=−69.0 kJ/mol. What is Δ? for this reaction at 298 K when the partial pressures are ?N2=0.500 bar, ?H2=0.150 bar, and ?NH3=0.750 bar? Show work please!
Which of the following reactions is a heterogeneous equilibrium expression? a. 2NO(g) + O2(g) 2NO2(g) b. 2NH3(g) N2(g) + 3H2(g) c. 2H2(g) + O2(g) 2H2O(g) d. 2S(s) + 302(g) 2503(g) e. C2H4(g) + H2(g) C2H6(g)
The change in entropy, ΔS°rxn, is related to the the change in the number of moles of gas molecules, Δngas. Determine the change in the moles of gas for each of the following reactions and decide if the entropy increases, decreases, or has little or no change. a) 2H2(g) +O2(g)->2H2O b)C2H4(g) +H2(g)-> C2H6(g) c) CH4(g) + 2O2(g) -> CO2(g)+2H2O(l) d) PCL5(s)--> PCL3(l) + CL2(g)
Indicate whether pH increases, decreases, or stays the same when each of the following is added: (a) NaC3H5O3 to a solution of HC3H5O3: ___________ (b) C3H7NH3Cl to a solution of C3H7NH2: ___________
For the following reaction, Kp = 2.8 ✕ 104 at 1630 K. H2(g) + Br2(g) equilibrium reaction arrow 2 HBr(g) What is the value of Kp for the following reactions at 1630 K? (a) HBr(g) equilibrium reaction arrow 1/2 H2(g) + 1/2 Br2(g) (b) 2HBr(g) equilibrium reaction arrow H2(g) + Br2(g) (c) 1/2H2(g) + 1/2 Br2(g) equilibrium reaction arrow HBr(g)
35) Given the equilibrium reaction at constant pressure: 2HBr(g) + 72.7 kJ = H2(g) + Br2(g) When the temperature is increased, the equilibrium will shift to the A) left, and the concentration of HBr(g) will decrease B) right, and the concentration of HBr(g) will decrease C) right, and the concentration of HBr(g) will increase D) left, and the concentration of HBr(g) will increase
NEED HELP ASAP 1-4 and has a question. 1) A chemical reaction that releases heat to the surroundings is said to be _AH at constant pressure. A) endothermic, positive B) endothermic, negative C) exothermic, positive D) exothermic, neutral E) exothermic, negative kJ of heat are transferred when 161.8 2) The value of AHº for the reaction below is -72 kJ. g of HBr is formed in this reaction. H2(g) + Br2 (g) → 2HBr (g) A) 54 B) 36 C)...
Question 9 (6 pts) How does a decrease in temperature affect the partial pressure of the underlined substance and the value for Keq for each of the following reactions? Explain your answer! a) C(graphite) + 2H2(g) CH4(g) ∆H0 = -75 kJ b) N2(g) + O2(g) 2NO(g) ∆H0 = 181 kJ c) P4(s) + 10Cl2(g) 4PCl5(g) ∆H0 = -1528 kJ