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Question

Question 1:

For the reaction 2HNO3 + Mg(OH)2 → Mg(NO3) 2 + 2H2O, how many grams of magnesium nitrate are produced from 4 grams of nitric acid, HNO3 ?

Round your answer to the nearest tenth. Do not round your answers until the last step of the problem. If you do, the computer might mark your answer incorrect and you will be asked to complete your second trial for this assessment.

Use the following molar masses:

Element	Molar Mass
Hydrogen	1
Magnesium	24
Nitrogen	14
Oxygen	16

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Question 2:

S   + 6 HNO3 --> H2SO4 + 6 NO2 + 2 H2O

In the above equation how many grams of water can be made when 9 grams of HNO3 are consumed?

Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.:

Element	Molar Mass
Hydrogen	1
Nitrogen	14
Sulfur	32
Oxygen	16

I am so desperate

Answer 1

From the balanced equation, we see that 1 mol of Mg(NO₃)₂ is produced for 2 moles of HNO₃. Since this is a "mass/mass" problem, you need the molar masses of each of these two compounds. Using the formulas & the atomic masses, we get 148 g/mol for the magnesium nitrate & 63 g/mol for the nitric acid. So,

(148 g Mg(NO₃)₂ / 1 mol Mg(NO₃)₂) (1 mol Mg(NO₃)₂ / 2 mol HNO₃) (1 mol HNO₃ / 63 g HNO₃) (4 g HNO₃)

= 46.98 = 47 g Mg(NO₃)₂

Following the same logic you can di the 2nd question.