B) 1/2 N2(g) + 2H2(g) + 1/2 Cl2(g) → NH4Cl(s) C) N2(g) + H2(g) + Cl2(g)...
Given the following information, N2(g) + 4 H2(g) + Cl2(g) 2 NH4Cl(s) H= -628.8 kJ what is the H if 13.8g of hydrogen gas is consumed in the reaction? A) -2.15x10^3 KJ B) -8.61x10^3 KJ C) -1.08x10^3 KJ D) -6.29x10^2 KJ
1) 2) 3) 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) N20(g) + H20(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) +H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO2 Ok[NO]2[H212 O k[NO]2[H2] Ok[N20][H2] k[NO]1/2[H2] 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045 0.045 concentration of Cl2(M) Rate (M/s) 0.01 3.40 x 10-4 8.50 x...
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s)+H2O(g)+heat⇌CO(g)+H2(g) Part C What effect does each of the following changes have on the equilibrium? Drag the appropriate stresses to their respective bins. add H2O, Add heat, lower temperature, remove CO Categories: Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift
Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6 kJΔH=−95.7 kJΔH=−184.6 kJ
Use the following reactions to find H when 1 mole of HCl gas forms from its elements: N2(g) + 3 H2(g) 2 NH3(g) H = 91.8 kJ N2(g) + 4 H2(g) + Cl2(g) 2 NH4Cl(s) H = 628.8 kJ NH3(g) + HCl(g) NH4Cl(s) H = 176.2 kJ
9) Which contains both polar and non-polar bonds? (1 point) a) NH4Cl b) HCN HỌC c) H202 mod d) CH4 e lo
Given: C(s) +2H2(g) → CH4(g) If Δ[CH4]/Δt = 7.2x10-4 M/s, then -Δ[H2]/Δt is equal to ________ M/s.
The rate law for the reaction 2H2(g) + 2NO(g) ----> N2(g) + 2H2O(g) is rate=k[H2][NO]2. What is the rate constant at 800 degrees C when [NO] = 0.050 M and [H2] = 0.010 M and the rate of the reaction is 1.5 M/s
Which ONE of the following samples contains the largest number of atoms? A) 1 g N2 B) 1 g Li C) 1 g Cl2 D) 1 g P4 E) 1 g Mg
Using the equations N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol C(s) + 2 H2 (g) → CH4 (g) AH° = -74.9 kJ/ mol H2 (g) + 2 C(s) + N2 (g) → 2 HCN (g) AH° = 270.3 kJ/mol Determine the enthalpy for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g).