Assuming the reaction is first order in sucrose, determine the mass of sucrose that is hydrolyzed when 2.50 L of a 0.130 M sucrose solution is allowed to react for 190 min .

Full Question:

The hydrolysis of sucrose C12H22O11 into glucose and fructose in acidic water has a rate constant of 1.8 x 10^-4 s^-2 at 25 C.

Assuming the reaction is first order in sucrose, determine the mass of sucrose that is hydrolyzed when 2.50 L of a 0.130 M sucrose solution is allowed to react for 190 minutes.

96.96g

Explanation:

t = 190 x 60 = 11400 s (upon conversion to seconds)

k = 1.8 x 10^-4 s^-2

ln[A] −ln[A]o = −kt

ln[A] = -kt + ln[A]o

ln[A] = - ( 1.8 x 10^-4  * 11400) + ln (0.130)

ln[A] = - 2.052 - 2.04

[A] = 0.0167M

initial moles = 2.50 x 0.130 = 0.325

moles after 190 min = 0.0167 x 2.50 = 0.04175

moles hydrolyzed = 0.325 - 0.04175 = 0.28325

mass = 0.28325 x 342.30 g/mol = 96.96g

i think a, hope it .

explanation:

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"