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Brut [27]
3 years ago
14

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is exce

ss NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.
Chemistry
1 answer:
Iteru [2.4K]3 years ago
5 0

Answer:

10.85 g of water

Explanation:

First we write the balanced chemical equation

3NO_{2} +H_{2}O -->2HNO_{3} +NO

Then we calculate the number of moles of nitric acid produced

n(HNO3) = \frac{mass}{molar mass} =\frac{75.9g}{63.02g/mol}=1.2044 mol

According to the balanced equation, water needed in moles is always half the number of moles of HNO3 produced. So since we will produce 1.2044 mol of HNO3, we will need 0.6022 mol of water. Now to calculate what mass that is:

mass(water)=number of moles*molar mass=0.6022mol*18.02g/mol=10.85g

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Answer:

C. increase to 7.

Explanation:

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In this case, the undergoing chemical reaction is:

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katen-ka-za [31]

Answer:

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Explanation:

The number of ions in 17.1 gm of aluminum sulphate Al2 (SO4)3 =….. [Molar mass of Al2 (SO4)3 = 342 gm]

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