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Vera_Pavlovna [14]
3 years ago
8

For the reaction 2HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are produced from 18.21 mol of nitric ac

id, HNO3?
a. 1350
b. 901
c. 5410
d. 1130
Chemistry
1 answer:
enyata [817]3 years ago
7 0
The answer is A. 1350

(ALL NUMBERS Except the grams is given from the equation)
18.21mol HNO3/1 * 1mol MgN206/2mol/ 2mol HNO3 * (molar mass-->)148.30 MgN206/ 1mol MgN2O6 

You multiply 18.21HNO3* 1mol MgN2O6 * 148.30MgN2O6
Then divide it by the 2mol HNO3 to get 1350

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3 0
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(LO 37,45) A reaction is 75% complete in 45.0 min. How long after its start will the reaction be 50% complete if it is (A) first
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Answer:

A) t = 22.5 min and B) t = 29.94 min

Explanation:

Initial concentration, [A]₀ = 100

Final concentration = 100 -75 = 25

Time = 45 min

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ln[A] − ln[A]₀ = −kt

Solving for k;

ln[25] − ln[100] = - 45k

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Initial concentration, [A]₀ = 100

Final concentration, [A] = 100 -50 = 50

Time = ?

ln[A] − ln[A]₀ = −kt

Solving for k;

ln[50] − ln[100] = - 0.0308 * t

-0.693 = -0.0308 * t

t = 22.5 min

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[A] = [A]₀ − kt

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25 = 100 - k(45)

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How long after its start will the reaction be 50% complete?

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Time = ?

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50 = 100 - (1.67)t

-50 = - 1.67t

t = 29.94 min

3 0
3 years ago
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