At 699 K, AG° = -23.25 kJ for the reaction H2(g) + 12(g) = 2 HI(g)....
Incorrect Question 1 0/1 pts At 699 K, AGⓇ = -23.25 kJ for the reaction H2 (9) + 12 (9) =2HI (9). Calculate AG for this reaction if the reagents are both supplied at 10.0 atm pressure and the product is at 2.00 atm pressure. -42.2kJ +4.5k +422 kJ +18.7 kJ .-18.7 kJ
15. At 699 K AG° = -23.25 kJ for the reaction H2g) + 12(a)= 2Hg). Calculate AS this reaction if the reagents are both supplied at 10.0 atm pressure and the pro is at 1.94 atm pressure A) -19.1 kJ B) 19.1 kJ C) 42 kJ D) 42 3 kJ E) 42 3 kJ
8. The AG for the reaction H2(g) + 12(e) = 2 HI) is 2.60 kJ/mol at 25°C. In an experiment, the initial pressures are Pe = 3.98 atm, P = 0.044 atm, and P = 0.29 atm. Calculate AG for the reaction and predict the direction of the net reaction
ΔGf°(I2(g)) = 19 kJ/mol 7. For the reaction H2(g) +12(g) = 2HI(g) K = 50.0 at 721 K (a) What is AG at 721 K? (b) What is Kat 25 °C? (AG HI(g) = +1.7 kJ/mol)
at 1000 K? for the reaction 12. The equilibrium constant, K 2 HI(g) H2(g) I2(g) is 55 at 425 C. Ifa 0.40 mol sample of HI was introduced into a 1.00 mL. reaction vessel at 425 C, what are the equibrium concentrations of H2, 12, and HI? 13. Consider the following reaction which is at equilibrium at 25 C 2 NH3(g) + CO2(g) A-152.2 kJ Ni4(NH2CO2X) In which direction will the reaction shift if (a) the pressure is increased (b)...
A student ran the following reaction in the laboratory at 690. K: H2(g) +12(g) 22HI(g) When he introduced H2(g) and 12(g) into a 1.00 L evacuated container, so that the initial partial pressure of H2 was 4.40 atm and the initial partial pressure of I was 3.28 atm, he found that the equilibrium partial pressure of HI was 5.78 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group...
For the reaction N2(g) + 3 H2(g) = 2 NH3(g), what is AG (in kJ) at 298 K when the pressures of the gases are: P(N2) .13 atm P(H2) = 6.2 x 10-5 atm P(NH3) = 1.8 atm? O +47.0 O-113 O-2.49 0 -33.0 O +1.73
Cls, graphite)+H2O (g)CO (B)+H2 (g) (a) Calculate AG for the reaction: where temperature is 700 K, AG° 92 kJ and the initial pressure of each gas is P H,0 = 0.67 atm, P co 0.23 atm, P H, = 0.51 atm. (b) What direction would this reaction proceed?
Find AG (in kJ mol-1 to one decimal place) for the following reaction at 198.15 K when Phi= 2.0 atm, Piz=5.0 atm, and PH2=3.0 atm. H2(g) +12(8) —HI(g)
The equilibrium constant, K., for the following reaction is 55.6 at 698 K. H2(g) +12(E) 2 HI(g) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I are introduced into a 1.00 L vessel at 698 K. M [H2 1 = [12] [HI] - M M