A Assuming the reaction is first order in sucrose, determine the mass of sucrose that is hydrolyzed when 2.50 LL of a 0.180 MM sucrose solution is allowed to react for 200 minmin .

The question is incomplete, here is the complete question:

The hydrolysis of sucrose into glucose and fructose in acidic water has a rate constant of 1.8×10⁻⁴ s⁻¹ at 25°C. Assuming the reaction is first order in sucrose, determine the mass of sucrose that is hydrolyzed when 2.65 L of a 0.120 M sucrose solution is allowed to react for 200 min.

The mass of sucrose solution left is 12.56 grams

Explanation:

Molarity is calculated by using the equation:

Molarity of sucrose solution = 0.120 M

Volume of solution = 2.65 L

Rate law expression for first order kinetics is given by the equation:

where,

k = rate constant =

t = time taken for decay process = 200 min = (200 × 60) = 12000 seconds

= initial amount of the sample = 0.318 moles

[A] = amount left after decay process = ?

Putting values in above equation, we get:

To calculate the mass from given number of moles, we use the equation:

Moles of sucrose = 0.0367 moles

Molar mass of sucrose = 342.3 g/mol

Putting values in above equation, we get:

Hence, the mass of sucrose solution left is 12.56 grams

calculate how many grams of ammonia can be produced from 4.21 grams of

n2 + 3h2 = 2nh3

my answer:

25.0g n2 x (1 mol/ 28.0gn2) x (2 mol nh3/ 1 mol n2) x (17.0g nh3/ 1 molnh3) = 30.36g n2

25.0g h2 x (1 mol h2/ 2.00g h2) x (2 mol nh3/ 3 mol h2) x (17.0g nh3/ 1 mol nh3) = 141.67g h2

lr = n2

the answer is a and have a great day