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rosijanka [135]
2 years ago
6

How many moles are equal to 89.23 g of calcium nitrate?

Chemistry
1 answer:
DanielleElmas [232]2 years ago
6 0

Answer:

23

Explanation:

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What mass of ammonia can be produced if 13.4 grams of nitrogen gas reacted ?
aivan3 [116]

Answer:

If 13.4 grams of nitrogen gas reacts we'll produce 16.3 grams of ammonia

Explanation:

Step 1: Data given

Mass of nitrogen gas (N2) = 13.4 grams

Molar mass of N2 = 28 g/mol

Molar mass of NH3 = 17.03 g/mol

Step 2: The balanced equation

N2 + 3H2 → 2NH3

Step 3: Calculate moles of N2

Moles N2 = Mass N2 / molar mass N2

Moles N2 = 13.4 grams / 28.00 g/mol

Moles N2 = 0.479 moles

Step 4: Calculate moles of NH3

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

For 0.479 moles N2 we'll produce 2*0.479 = 0.958 moles

Step 5: Calculate mass of NH3

Mass of NH3 = moles NH3 * molar mass NH3

Mass NH3 = 0.958 moles * 17.03 g/mol

Mass NH3 = 16.3 grams

If 13.4 grams of nitrogen gas reacts we'll produce 16.3 grams of ammonia

3 0
3 years ago
Why are silver, lead, and mercury so special? (why do they always precipitate out and never dissolve) PLEASE BE DETAILED BUT SIM
lara [203]
Silver and lead are special elements, where silver is insoluble in all halogen anions (like AgCl, AgI, AgBr)
and lead is insoluble in sulphates and halogen anions ( PbSO4, PbCl2, etc.)
Mercury is special because it is the only metal that is a liquid at room temperature
hope this helps!!
8 0
3 years ago
What is the definition of solute
sdas [7]

Answer:

a substance that can be dissolved by a solvent to create a solution

Explanation:

8 0
2 years ago
Read 2 more answers
Lance wants to separate out the salt from a solution of salt water how can he do this
qwelly [4]

*☆*――*☆*――*☆*――*☆*――*☆*――*☆*――*☆*――*☆**☆*――*☆*――*☆*――*☆

Answer: Boiling the water

I hope this helped!

<!> Brainliest is appreciated! <!>

- Zack Slocum

*☆*――*☆*――*☆*――*☆*――*☆*――*☆*――*☆*――*☆**☆*――*☆*――*☆*――*☆

4 0
2 years ago
Calculate the mass of oxygen gas (O2) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the
Ilia_Sergeevich [38]

Answer:

The mass of oxygen gas dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 0.04936 grams.

Explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

To calculate the molar solubility, we use the equation given by Henry's law, which is:

C_{gas}=K_H\times p_{gas}

where,

K_H = Henry's constant =

p_{O_2} = partial pressure of oxygen

We have :

Pressure of the air = P

Mole fraction of oxygen in air = \chi_{O_2}=0.210

p_{O_2}=P\times \chi_{O_2}

=0.210\times 1.13 atm= 0.2373 atm

K_H = Henry's constant = 1.30\times 10^{-3}M/atm

Putting values in above equation, we get:

C_{O_2}=1.30\times 10^{-3}M/atm\times 0.2373  atm\\\\C_{O_2}=0.003085 M

Moles of oxygen gas = n

Volume of water = V = 5 L

Molarity = \frac{Moles}{Volume(L)}

0.003085 M=\frac{n}{5 L}

n = 0.003085 M\times 5 L=0.001542 mol

Mass of 0.001542 moles of oxygen gas:

0.001542 mol × 32 g/mol = 0.04936 g

The mass of oxygen gas dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air is 0.04936 grams.

5 0
2 years ago
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