19. The expression for the reverse reaction: NH4NO2 (s)
<--> N2 (g) + 2H2O is:
a. Keq = [N2] [H2O] ^ 2
b. Keq = [NH4NO2] / [N2] [H2O] ^ 2
c. Keq = [N2] [H2O] ^ 2 / [NH4NO2]
d. Keq = 1 / [N2] [H2O] ^ 2
19. The expression for the reverse reaction: NH4NO2 (s) <--> N2 (g) + 2H2O is: a....
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g), what direction will the reaction proceed if [NO]=7.9x10-3M, [H2]=0.25 M, [N2]=0.15 M, & [H2O]=0.13 M. (K=650) forward reverse the reaction has stopped the reaction is at equilibrium
Which reaction is accompanied by an increase in entropy? A N2(g) + 3 H2(g) – 2 NH3(g) B. Ba(OH)2(s) + CO2(g) → BaCO3(s) + H2O(1) C. NH4NO2(s) – N2(g) + 2 H20(0) D.2 C2H2(g) + 5 O2(g) – 4 CO2(g) + 2 H2O(s) E. C8H16(1) + 12 O2(g) — 8 CO2(g) + 8 H 20(1)
What is the total volume of products obtained when 128 g NH4NO2 decomposes at 819 o C and 2.00 atm NH4NO2 (s) → N2 (g) + 2H2O (g)
Ammonium nitrite, NH4NO2, decomposes upon heating to form N2 gas according to the following balanced chemical equation. When a sample of NH4NO2 was decomposed in a test tube, 813.9 mL of N2 gas was collected over water at 47.64 °C and the total pressure was 765.9 torr. NH4NO2(s) → N2(g) + 2 H2O(l). How many grams of N2 were collected?
QUESTION 9 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187.8 kJ
1. 2. Consider the reaction 2NO(g) + 2H2(g)—>N2(g) + 2H2O(1) Based upon the stoichiometry of the reaction the sign of ASørxn should be positive Using standard thermodynamic data, calculate AS rxn at 25°C. AS rx = J/Kºmol Using values of AG calculate AGºrx for the following reaction. Is the reaction product favored or reactant-favored? SICI(g) + 2 Mg(s) + 2 MgCl2(s) + Si(s) AG°(kJ/mol) HgS(s) -50.6 SO2(g) -300.13 H2S() -33.56 H20() -228.59 SiCl() -622.76 MgCl2() -591.59 kJ/mol O product-favored reactant-favored
2. Determine which of these reaction(s) are redox reaction. 6 Li2O(s) + P4010(g) → 4 Li3PO4(s Cao(s) + H2O(1) + Ca(OH)2(s) s(s) + 3 F2(g) → SF6(g) Zns(s) + 2 O2(g) → ZnSO4(s) SO2(g) + Cl2(g) → SO2Cl2(g) CuSO4.5H20(s) → CuSO4(s) + 5 H2O(g) SnCl4•6H2O(s) → SnOz(s) + 4 HCl(8) + 4 H20(8) NH4NO2(s) → N2(g) + 2 H2O(g) (NH4)2Cr207(s) → N2(g) + Cr2O3(s) + 4 H2O(g) 2 Na(s) + Cl2(g) → 2 NaCl(s) SO3(g) + Cao(s) > CaSO4(s) SO2(g)...