Consider the following reaction: 2 NO_2(g) + Br_2(g) → 2 NO_2Br(g)
What is the rate constant k?
Consider the following reaction: 2 NO_2(g) + Br_2(g) → 2 NO_2Br(g) What is the rate constant...
The following initial rate information was collected at 25°c for the following reaction: 2H2(g)+2NO(g) N2(g) +2H20(g) H2lo (M) INOlo (M) Initial Rate (M/min) 0.0010 0.0020 1.2 x 10-4 0.0010 0.0030 1.8 x 104 0.0020 0.0020 4.8 x 104 Determine the overall order of the reaction and present you answer in numeric torm (le. 0, 1,2 eto)
The rate equation for the reaction 2NO(g) + Br_2(g) rightgarrow 2NOBr(g) was determined experimentally to be: Rate = k[NO]^2 [Br_2] Five possible mechanisms have been proposed (i)-(v). Determine the rate equation for each mechanism below and then decide with reasons, (based on the information given) which mechanism is the most likely. (i) 2NO (g) + Br_2 (g) rightarrow 2NOBr (g) (ii)NO (g) + Br_2 rightwardsharpoonoverleftwardsharpoon NOBr_2 (g) NOBr_2 (g) + NO (g) rightarrow 2NOBr (g) (iii) Br_2 rightwardsharpoonoverleftwardsharpoon Br +...
For the reaction H_2(g) + Br_2 (g) rightarrow 2HBr(g) K_p = 3.6 times 10^4 at 1496 K. What is the value of K'_p for the following reaction at 1496 K? HBr(g) rightarrow 1/2 H_2(g) + 1/2 Br_2(g) K'_p =
Consider the following reaction mechanism: step 1: 2 NO_2 rightarrow NO + NO_3 step 2: NO_3 + CO rightarrow NO_2 + CO_2 What intermediate is involved in this mechanism? NO_2 NO NO_3 CO CO_2 Consider the reaction given below: 2 A(g) + 3 B(g) 2 C(g) delta H = 12.5 kJ/mol K_p = 10.0 If a reaction mixture has the following partial pressures: P_A = 1.0 atm P_B = 2.0 atm P_C = 2.0 atm which of the following statements...
Experimental rate data for the reaction 2H2(g) + Cl2(g) → 2HCl(g) are given in the chart below. Experiment [H2] [Cl2] Rate in M×s-1 1 0.0020 0.0075 3.8 x 10-3 2 0.0020 0.0025 1.3 x 10-3 3 0.0050 0.0025 1.3 x 10-3 4 0.0050 0.0010 0.5 x 10-3 a). What are the orders of the reaction for H2 and Cl2 individually? SHOW WORK. b).Then write the rate law for this overall reaction:
Given the following data for this reaction CH3Cl(g) + 3 Cl2(g) --> CCl4(g) + 3 HCl(g) Trial [CH3Cl]i, M [Cl2]i, M Initial rate of reaction, M/s 1 0.010 0.0010 2.40 × 10-4 2 0.010 0.0030 2.16 × 10-3 3 0.020 0.0030 1.73 × 10-2 4 0.0050 0.010 ? What is the initial rate of disappearance of Cl2 in trial #4? 8.70 10-4 M/s 4.50 10-3 M/s 3.00 10-4 M/s 9.00 10-3 M/s
The equilibrium constant K_c for the reaction H_2 (g) + Br_2(g) 2 HBr(g) is 2.180 times 10^6 at 730 degree C. Starting with 2.20 moles of HBr in a 21.6-L reaction vessel, calculate the concentrations of H_2, Br_2 and HBr at equilibrium. [H_2] = [Br_2] = [HBr] =
Be sure to answer all parts. The equilibrium constant K_c for the reaction H_2(g) + Br_2(g) = 2HBr(g) is 2.180 Times 10^6 at 730DegreeC. Starting with 5.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H_2, Br_2, and HBr at equilibrium. [H_2] = M [Br_2] = M [HBr] = M
Consider the following reaction: 2HBr (g) rightarrow H_2 (g) + Br_2 (g) In the first 23.0 s of this reaction the of HBr dropped from 0.550 M to 0.457 M. Calculated the average rate of the reaction in this time interval. Express your answer using two significant figures. If the volume of the reaction in part (b) was 1.50 L. what amount of Br_2 (in moles) was formed during the 15.0 is of the reaction? Express your answer using two...
Consider the following chemical reaction, at 500degree C and 200atm, for question 1-5: Step1: NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) Step 2: NO_2(g) + F_2(g) rightarrow NO_2F(g) rate determining step After this two-step process occurs, what is the overall balanced chemical equation? NO_2(g) + F_2(g) rightarrow NO_2F(g) + F(g) NO_2(g) + F_2(g) rightarrow NO_2F(g) + F_2(g) 2NO_2(g) + F_2(g) rightarrow 2NO_2F(g) 2NO_2(g) + F_(g) rightarrow 4NO_(g) + F(g) What is the intermediate this multistep mechanism? NO_2(g) F_(g) NO_2F_(g) F_2(g)...