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11 Nov 2019

The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose we start with 2.40×10−2 mol of N2O5(g) in a volume of 1.9 L . How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol ?

What is the half-life of N2O5 at 70∘C?​

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Sixta Kovacek
Sixta KovacekLv2
6 Nov 2019

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Related questions

Section 1:

The first-order rate constant for the decomposition of N2O5,
2N2O5(g)→4NO2(g)+O2(g),
at 70∘C is 6.82×10−3s−1. Suppose we start with 2.80×10−2 mol of N2O5(g) in a volume of 1.5 L .

a) How many moles of N2O5 will remain after 7.0 min?

b) How many minutes will it take for the quantity of N2O5 to drop to 2.0×10−2 mol?

Section 2:

Consider the following hypothetical aqueous reaction: A(aq)→B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected:

Time (min) 0 10 20 30 40
Moles of A 0.065 0.051 0.042 0.036 0.031

What is the half-life for the reaction?

The first-order rate constant for the decomposition of N2O5, givenbelow, at 70°C is 6.82 10-3 s-1. Suppose we start with 0.0150 molof N2O5(g) in a volume of 3.0 L.

2 N2O5(g) ? 4 NO2(g) + O2(g)

(a) How many moles of N2O5 will remain after 3.5 min?
mol

(b) How many minutes will it take for the quantity of N2O5 to dropto 0.005 mol?
min

(c) What is the half-life of N2O5 at 70°C?
min

The first-order rate constant for the decomposition of N2O5,
2N2O5(g)?4NO2(g)+O2(g),
at 70?C is 6.82�10?3s?1. Suppose we start with 3.00�10?2mol of N2O5(g) in a volume of 2.5L .

A) How many moles of N2O5 will remain after 7.0min ?

Express your answer using two significant figures.

B) How many minutes will it take for the quantity of N2O5 to drop to 1.1�10?2mol ?

Express your answer using two significant figures.

C) What is the half-life of N2O5 at 70?C?

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