A sample of 0.900 mol N2O is placed in a sealed container, where it decomposes irreversibly to N2and O2 in a first-order reaction (2N2O   .→    2N2   +  O2). After 42.0 min, 0.640 mol N2O remains.  How long will it take for the reaction to be 90.0% complete

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.00717s CICH,CH,C1 (g) → CH,CHC1 (g) +HC1 (g) Suppose a vessel contains CICH,CH,Cl at a concentration of 1.00 M. Calculate the concentration of CICH,CH,Cl in the vessel 89.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

A first-order reaction has rate constant, k = 0.217 min-1. What is the half-life for the reaction? 1.81 min 2.24 min 2.78 min 4.61 min 3.19 min

H2O2 decomposes according first order kinetics. If the rate constant is 1.00 x 10-3 minutes-1 , calculate the length of time, in minutes, for 60% of the sample to decompose.

Consider this reaction: 2HI (g) → H₂(g) + 1₂ (g) At a certain temperature it obeys this rate law. -1 2 rate = (1.06 M¹s¹) [HI] ² S Suppose a vessel contains HI at a concentration of 0.510M. Calculate how long it takes for the concentration of HI to decrease to 0.0561 M. You may assume no other reaction is important. Round your answer to 2 significant digits. x10 X

A first-order reaction has a half-life of 25.5 s. How long does it take for the concentration of the reactant in the reaction to fall to one-sixteenth of its initial value? Express the time to three significant figures and include the appropriate units. HẢ ? t = Value Units

At a certain temperature the rate of this reaction is second order in NH4OH with a rate constant of 0.0770M NH₂OH(aq) → NH3(aq) + H₂O (aq) Suppose a vessel contains NH4OH at a concentration of 0.500M. Calculate how long it takes for the concentration of NH4OH to decrease by 77.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 : x10

The reaction 2 A(g) -->  A(g) obeys zero-order kinetics. The reaction begins with 5.57E2 g of A. After 8.57E0 minutes 1.93E2 g of A remains. What is the half-life for this reaction in minutes?

At a certain temperature this reaction follows first-order kinetics with a rate constant of 7.29 x 10 s : 2SO3 (g) -2S0, (g) +0, (g) Suppose a vessel contains SO, at a concentration of 1.45M. Calculate the concentration of SO, in the vessel 850. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

A compound with the formula, C3H6 undergoes an isomerization reaction in the gas phase to form a new compound with the same molecular formula. The isomerization reaction is first-order with a rate constant of 5.87 x 10-4 sec-1 at 485 degrees Celsius. If a 2.50 liter flask initially contains 722 torr of the starting gaseous compound at 485 degrees Celsius, how long will it take, in minutes, for the partial pressure of the starting compound to drop below 1.00 x 102 torr?