The following data was collected for the reaction between hydrogen and nitrogen

Question

The following data was collected for the reaction between hydrogen and nitrogen monoxide. The time recorded corresponds to a N_2 concentration change of 5.3 times 10^-4 M. 2H_2(g) + 2NO(g) times 2H_2 O(g) + N_2(g) a. Calculate the reaction rate for each of the three trials. b. Determine the order of the reaction with respect to H_2. c. Determine the order of the reaction with respect to NO. d. What is the rate law for this reaction? e. What is the rate constant? In the reaction being studied this week, what chemical is being used measure reaction time? What are we using as an indicator? Calculate the initial reactant concentrations for each of the trials in Pt I. [I^-] after mixing A & B (M) [S_2O_8^2-] after mixing A & B (M) Show your work from Trial I.

Explanation / Answer

ANSWER=

1 RATE OF REACTION =CHANGE IN CONCENTRATION /CHANGE IN TIME

INITIAL 37 SEC START TIME PLEASE TABLE USE ACCORDING TO TIME OR SETUP 37 SEC 74 SEC THAN 296 SEC

1 37 SEC NO CHENGE IN CONCENTRATION OR TIME SO ===0.02/37 ==>5.40X10-4 MOLE/SEC

2 74 SEC ==>CHANGE IN CONCENTRATION [0.02-0.01=0.01]/CHANGE IN TIME [74-37=37]==>0.01/37=>2.7X10-4 MOLE/SEC

3 296 SEC ===> REACTION COMPLTE NO CHANGE IN CONCENTRATION =>0/296=> 0 RATE OF REACTION ZERO REACTION NOT PROCEED IT CAN SAY COMPLTE

2 AND 3...ORDER OF REACTION H2 AND N2 RESPECT BOTH ARE ZERO ...

4..RATE LAW ==K [H2]0 [NO]0

5.RATE CONSTANT =K0=X/T 0.01/37==>2.7X10-4 MOL LITER-1SEC-1

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