Consider the following balanced equation: 4 NH_3 (g) + 3 O_2 (g) right arrow 2 N

Question

Consider the following balanced equation: 4 NH_3 (g) + 3 O_2 (g) right arrow 2 N_2 (g) + 6 H_2O (1) During a certain time interval, the average rate of disappearance of O_2 was equal to 4.50 * 10^-3M/s. Which of the following represents the average rate of disappearance of NH_3 during this time interval 1.50 * 10^-3 M/s 3.38 * 10^-3 M/s 6.00 * 10^-3 M/s 1.80* 10^-2 M/s 2.50 * 10^-2 M/s The decomposition of H_2O_2 in the presence of 1^-1 is believed to occur via the following mechanism: Step 1: H_2O_2 (aq) + 1^- (aq) right arrow H_2O (I) + IO^- Step 2: H_2O_2 (aq) + IO^- (aq) right arrow H_2O (I) + (g) + I^-1(aq) Which of the following is true of this mechanism 1^- and IO^- are both intermediates I^- and IO^- are both catalysts I^- is an intermediate, and IO^- is a catalyst I^- is a catalyst, and IO^- is an intermediate

Explanation / Answer

Answer; According to the given informations of the question we know that rates are equal hence,

the rate of disappearence of O2 = 1/3 d[O2] /dt = 4.50 * 10-3 = 1/4 dNH3 /dt

Hence the rate of disappearence of NH3 = 4 * 4.50 * 10-3 M/s

= 1.8 * 10-2 m/ s

Hence the rewuired answer is option [d] .

2] According to the given informations Here we can observe that I- is participating in the reaction and in the final state it is release means it act as a catalyst .

So the correct option is [d] I- is a catalyst and IO- is Intermediate .

Hence it is all about the given question thank you :)

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