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Anna35 [415]
3 years ago
13

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 w

ith 2.00×10−2 mol of n2o5(g) in a volume of 2.3 l . you may want to reference (page) section 14.4 while completing this problem. part a how many moles of n2o5 will remain after 4.0 min ?,
Chemistry
1 answer:
torisob [31]3 years ago
7 0

The rate constant for 1st order reaction is

K = (2.303 /t) log (A0 /A)

Where, k is rate constant

t is time in sec

A0 is initial concentration

(6.82 * 10-3) * 240 = log (0.02 /A)

1.63 = log (0.02 /A)

-1.69 – log A = 1.63

Log A = - 0.069

A = 0.82

Hence, 0.82 mol of A remain after 4 minutes.

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Empirical formula for compound of 2.17 mol N and 4.35 mol O
balu736 [363]

Answer:

Explanation:

ratio of  moles of N and O in molecule =

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4 0
2 years ago
What properties of matter are intensive independent of their size
Paha777 [63]

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temperature, refractive index, density, and hardness of an object

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3 years ago
W7L5 Stoichiometry Practice 2
Rzqust [24]

Answer:

.079 moles of Nirogen gas (N2)

Explanation:

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      One half as many moles of N2 are needed  = .079 moles

6 0
2 years ago
SO2 + H2O = H2SO3 and not H2SO4?
kramer
It's because the Law of Conservation of Mass WILL NOT be followed if, from SO2 and water, sulfuric acid is formed. Making a balanced chemical reaction is not possible, no matter what you do. To obtain or make sulfuric acid, SO2 still needs to be oxidized further to SO3.
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