CO(g) + H2(g) ---------------> C(g) + H2O(g)
reactants total volume = 2
products total volume = 2
in this reaction reactant volume and products volume are equal. It is not change the equilibrium when volume is changes.
10. 3O2(g) ------------> 2O3(g) endothermic reaction
pressure increases shift product side
Decrease the O2 gas shift to reactants side
The endothermic reaction takes place at high temperature.
Increases the temperature shift product side
Removal of the O3 shift product side
Decrease the O2 gas >>>>answer
9. Which of the following will have no shift in equilibrium if the volume is decreased?...
Predict the effect of decreasing the volume of the container for each equilibrium and why. a.) 2H2O (g) + N2 (g) <--> 2H2 (g) + 2NO (g) b.) SiO2 (s) + 4HF (g) <--> SiF4 (g) + 2H2O c.) CO (g) +H2 (g) <--> C (s) + H2O (g)
) Predict the effect of increasing pressure for each of the following equilibriums: (a) 2H2O (g) + N2 (g) ↔ 2H2 (g) + 2NO (g) ________________________ (b) SiO2 (s) + 4HF (g) ↔ SiF4 (g) + 2H2O (g) ________________________ (c) CO (g) + H2 (g) ↔ C(s) + H2O (g) __
N2+2H2O <--> 2NO =2H2. which way would the equilibrium shift if you remove H2?
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)
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
Given the following regression lines, calculate T_i and T_f if a reactant was added at t=3.5 min T= 0.10013*t + 16.46245 T= -0.14998*t + 30.00143 Which equation is used to calculate T_i? Which is used to calculate T_f? Calculate T_i and T_f Calculate Hfor the reaction: NH3(g)+5O2(g)->4NO(g)+6H2O(g) N2(g)+O2(g)->2NO(g) N2(g)+3H2(g)->2NH3(g) 2H2(g)+O2(g)->2H2O(g) Compound Hf(kJ/mol) H2(g) 0.00 H2O(g) -241.83 N2(g) 0.00 NH3(g) -45.94 NO +90.2 O2(g) 0.00 What’s the purpose of a calibration curve? What causes absorption?
N2+2H2O ,--> 2NO+2H2. which way would the equilibrium shift if you increased the volume?
17.51 Calculate the entropy change for the following processes. (a) 1.00 mol H,O(s) melts at 0 °C. AH = 6.01 kJ/mol. (b) 2.00 mol CH.() vaporizes at 80.0 °C. AH vap = 30.7 kJ/mol. 17.52 - Calculate the entropy change for the following processes. (a) 2.00 mol NH3(e) vaporizes at -33.0 °C. AHvap = 23.35 kJ/mol. (b) 1.00 mol C,H,OH(s) melts at -114 °C. AHjus = 5.0 kJ/mol. 17.53 Use data from Appendix G to calculate the standard entropy change...
1) Find the AH of the following reaction: C(s) + O2(g) à CO2(g) Given the following data: Sro(s) + CO2(g) à SrCO3(s) 2Sro(s) à 2Sr(s) +0,(8) AH = -234 kJ AH = +1184 kJ 2SCO,(s) à 25r(s) + 2C(s) + 302(g) AH = +2440 kJ 2) Find the AH of the following reaction: 3NO,(g) + H2O(l) à 2HNO,(aq) + NO(g) Given the following data: 2NO(g) + O2(g) à 2NO(g) AH=-116 kJ 2N2(g) + 502(g) + 2H2O(l) à 4HNO3(aq) AH =...
9. The following equilibrium is endothermic. In the box below, show how the reaction will shift response to the indicated stress by writing →., or no shift. 30,(8) 203(g) Stress Equilibrium shift? Increase O2 concentration Add heat Add a catalyst Cool reaction Benzene Bromine Bromobenzene Hydrogen bromide