1
answer
0
watching
243
views
18 Nov 2019
The first order reaction. SO_2cl_2 (g) rightarrow SO_2 (g) + Cl_2(g), has a rate constant equal to 2.20 times 10^-3 s^-1 at 593 K. What percentage of the initial amount of SO_2Cl_2 (g) will remain after 6.00 hours? In aqueous solution, hypobromite ion, BrO; reacts to produce bromate ion. BrO_3^-, and bromide ion, Br, according to the following chemical equation A plot of 1/[BrO^-] vs time is linear and the slope Is equal to 0.056 M^-1 s^-1. If the initial concentration of BrO^- is 0.80 M, how long will it take one half of the BrO^- ion to react? 3 BrO^+ (aq) rightarrow BrO_3^- (aq) + 2Br^- (aq). Express the equilibrium constant for the following reaction Pb(NO_3)_2 (aq) + 2 Nal(aq) Pbl_2 (s) + 2 NaNO_3 (aq) The reaction below has a K_p value of 3.3 times 10^8 What is the value of K_g for this reaction at 700 K? 2 SO_2 (g) 2 SO_2 (g) + O_2 (g) Consider the following reaction A reaction mixture initially contains 2.24 atm X_e and 4.27 atm F_2. If the equilibrium pressure of X_e is 0 34 atm, find the equilibrium constant (K_p) for the reaction. X_e(g) + 2F_2(g) X_eF_4(g)
The first order reaction. SO_2cl_2 (g) rightarrow SO_2 (g) + Cl_2(g), has a rate constant equal to 2.20 times 10^-3 s^-1 at 593 K. What percentage of the initial amount of SO_2Cl_2 (g) will remain after 6.00 hours? In aqueous solution, hypobromite ion, BrO; reacts to produce bromate ion. BrO_3^-, and bromide ion, Br, according to the following chemical equation A plot of 1/[BrO^-] vs time is linear and the slope Is equal to 0.056 M^-1 s^-1. If the initial concentration of BrO^- is 0.80 M, how long will it take one half of the BrO^- ion to react? 3 BrO^+ (aq) rightarrow BrO_3^- (aq) + 2Br^- (aq). Express the equilibrium constant for the following reaction Pb(NO_3)_2 (aq) + 2 Nal(aq) Pbl_2 (s) + 2 NaNO_3 (aq) The reaction below has a K_p value of 3.3 times 10^8 What is the value of K_g for this reaction at 700 K? 2 SO_2 (g) 2 SO_2 (g) + O_2 (g) Consider the following reaction A reaction mixture initially contains 2.24 atm X_e and 4.27 atm F_2. If the equilibrium pressure of X_e is 0 34 atm, find the equilibrium constant (K_p) for the reaction. X_e(g) + 2F_2(g) X_eF_4(g)
Sixta KovacekLv2
27 Jan 2019