Theroa tion X4 Y? ? sso ordorder with rospot toXard frst o dor with Oa Rate- km

Question

Theroa tion X4 Y? ? sso ordorder with rospot toXard frst o dor with Oa Rate- km spottoYwhic h of the lolo ingto the co to proason for the ratio Oe Rate k2XM QUESTION 2 For the reaction described in question 1, what is the effect on the rate of halving the concentration of X O a. It is doubled O b. It is halved. O c. It is quadrupled. O d. It is quartered. ?e.lt is the same. QUESTION 3 For the reaction A +BC, the rate law is rate = k[A] ?fthe initial concertration of A-1.9mon., the initial [B1-1:4 mol/L, ard the rate-0.48 moles of product per lire per minute Mmna Calculate the rate constant k to 2 decimal places QUESTION 4 In the reaction between H202 and 15 ml of 0.30M KI, 74. mL of 0.10M H202 and 21 mL of 0.020M Na2S203 were mixed in a flask containing starch and buffer and the total volume was made up to 500ml, with distilied water. The solution turned blue (ndicating the presence of l2) in 1.9 minutes. Calculate the initial rate of disappearance of H202 in units of M min-1 to two significant figures. (enter value in decimal form) Hint: theve are two reactions occuring here as represented by the equations 1 and 4 in the introduction of the lab manual procedure for this experiment

Explanation / Answer

Ans 1 is right

Ans 2

New concentration of X = X/2

Put X/2 in place of X, new rate

New Rate = k [X/2]2[Y]

New Rate = (1/4) k [X]2[Y]

New Rate = (1/4) Rate

1/4 of the original rate

It is quartered.

Option D is the correct answer

Ans 3

Rate = k[A]

It is first order reaction

[A] = 1.9 mol/L = 1.9 M

Rate = 0.48 M/min

Rate constant k = rate / [A]

= (0.48 M/min) / (1.9 M)

= 0.25 min-1

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