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The first-order rate constant for the decomposition of N₂O₁. 2N₂ Os (g) 4NO₂(g) + O₂(g) at 70° C is 6.82 x 10-3¹ Suppose we start with 2.10x10-2 mol of N₂Os (g) in a volume of 24 L Part B How many minutes will it take for the quantity of N₂O, to drop to 1.7x10-2 mol ? Express your answer using two significant figures. VAXO 3 1.1 The To Submit Previous Answers Request Answer GVC ? Part C min * Incorrect; Try Again; 2 attempts remaining Using the equation for a first-order reaction gives In A), kt+In Ale. Since the molarity is the number of moles per liter, the following relationship between the remaining number of moles (n.) and the initial number of moles (no) can be derived: The To where it is the rate constant (in inverse seconds) and t is the time (in seconds). Use the relationship to solve for time.
The first-order rate constant for the decomposition of N₂O₁. 2N₂O(g) +4NO₂(g) + O₂(g) at 70° C is 6.82 x 10³¹. Suppose we start with 2.10x10-2 mol of N₂Os (g) in a volume of 24 L X Incorrect; Try Again; 2 attempts remaining Using the equation for a first-order reaction gives In A-kt+In[A]. Since the molanty is the number of moles per liter, the following relationship between the remaining number of moles (,) and the initial number of moles (no) can be derived: T = noe where k is the rate constant (in inverse seconds) and t is the time (in seconds). Use the relationship to solve for time. Part C What is the half-life of N₂Os at 70°C? Express the half-life in seconds to three significant digits. t₁/2 = 19Η ΑΣΦΑ Submit Request Answer ?
The first-order rate constant for the decomposition of N₂O₂. 2N₂O(g) +4NO: (g) + O₂(g) at 70° C is 6.82 x 10³ Suppose we start with 2.10x102 mol of N₂O(g) in a volume of 24 L Part A How many moles of N₂O; will remain after 7.0 min ? Express the amount in moles to two significant digits. - 1.2x10-3 mol Previous Answers Correct The rate of reaction depends on the current concentration of the reactant(s). At a constant volume, the number of moles can be equated to the concentration, and the relationship among the initial number of moles ( ne), time (f), the number of moles at time t (ne), and the rate constant (k) for a first-order reaction is as follows: Part B In N₂Os] = -kt + In(n)= -kt + To solve for the number of moles at time t, we apply the relationship between the natural log and e to derive the following equation In N₂O) In(ne) T = n₂e How many mindes will it take for the many N.O. in den to 1 710 mal ?