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Mashutka [201]
3 years ago
8

I PLEASE HELP! How many liters of a 2.25 molar hydrobromic acid (HBr) solution would be needed to react completely with 100.0 gr

ams of calcium metal? Ca (s) + 2HBr (aq) CaBr2 (aq) + H2 (g)
Chemistry
1 answer:
PtichkaEL [24]3 years ago
8 0
Moles of calcium metal used = 100/40.1=2.5
Moles of HBr need to react = 5 moles 
As the molar ratio is 1 is to 2 among them 
so
Moles=molarity x volume
5=2.25 x volume
volume=2.22 litres of HBr required for this reaction
ANSWER IS 2.22 LITRES
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Answer: Option (d) is the correct answer.

Explanation:

According to the given situation, mass of compound will be calculated as follows.

Mass of compound = mass of flask and condensed vapor - mass of flask

                                 = 115.23 - 114.85

                                = 0.38 g

Volume (V) = 255 mL = 255 \times 10^{-6} m^{3}        (as 1 ml = 10^{-6} m^{3})

Pressure (P) = 101325 Pa

Temperature = 100^{o}C = (100 + 273) K = 373 K

Now, according to the ideal gas equation, PV = nRT

and, moles of compound n = \frac{PV}{RT}

                     = \frac{101325 \times 255 \times 10^{-6}}{8.314 \times 373}

                     = 0.008332 mol

As, molar mass of compound = \frac{mass}{\text{no. of moles}}

                                                  = \frac{0.38}{0.008332}

                                                  = 46 g/mol

Therefore, the compound is C_{2}H_{5}OH (molar mass = 12 x 2 + 5 x 1 + 16 + 1 = 46 g/mol).

Thus, we can conclude that out of the given options the liquid could be C_{2}H_{5}OH.  

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Answer:

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Explanation:

reaction is

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