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Sever21 [200]
1 year ago
14

How many grams of hno3 would you need to prepare 5.5 l of this solution

Chemistry
1 answer:
k0ka [10]1 year ago
3 0

8305 grams of HNO3 would be needed to prepare 5.5L of a solution. Details on how to calculate mass is found below.

<h3>How to calculate mass?</h3>

The mass of a substance in a solution can be calculated using the following formula:

Density = mass ÷ volume

According to this question, 5.5L of a HNO3 solution is given.

Density of HNO3 is 1.51 g/cm³

Volume of HNO3 = 5500mL

1.51 = mass/5500

mass = 8305g

Therefore, 8305 grams of HNO3 would be needed to prepare 5.5L of a solution.

Learn more about mass at: brainly.com/question/19694949

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<h3>                       ∴  1s²2s²2p⁶ is the noble gas (neon)</h3>

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List the official SI units
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Answer:

The seven SI base units, which are comprised of:

Length - meter (m)

Time - second (s)

Amount of substance - mole (mole)

Electric current - ampere (A)

Temperature - kelvin (K)

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Explanation:

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What will happen if you take a frog out of the food chain?
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4 0
3 years ago
How many grams of NH3 can be produced from 2.51 mil of N2 and excess H2 ?
salantis [7]

Answer:

85.34g of NH3

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

N2 + 3H2 —> 2NH3

Step 2:

Determination of the number of moles of NH3 produced by the reaction of 2.51 moles of N2. This is illustrated below:

From the balanced equation above,

1 mole of N2 reacted to produce 2 moles of NH3.

Therefore, 2.51 moles of N2 will react to produce = (2.51 x 2)/1 = 5.02 moles of NH3.

Therefore, 5.02 moles of NH3 is produced from the reaction.

Step 3:

Conversion of 5.02 moles of NH3 to grams. This is illustrated below:

Molar mass of NH3 = 14 + (3x1) = 17g/mol

Number of mole of NH3 = 5.02 moles

Mass of NH3 =..?

Mass = mole x molar Mass

Mass of NH3 = 5.02 x 17

Mass of NH3 = 85.34g

Therefore, 85.34g of NH3 is produced.

3 0
2 years ago
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