How many liters of a 2.25 molar hydrobromic acid (hbr) solution would be needed to react completely with 100.0 grams of calcium metal?

ca (s) + 2hbr (aq) cabr2 (aq) + h2 (g)

2.22 L

Explanation: To calculate the moles, we use the equation:

   ....(1)

For calcium:

Mass of calcium given = 100 g

Molar mass of calcium = 40 g/mol

Putting values in above equation, we get:

For the given reaction:

By Stoichiometry of the reaction,

1 mole of calcium reacts 2 moles of hydrogen bromide

So, 2.5 moles of calcium will react with = of hydrogen bromide.

Molarity is defined as the number of moles of solute dissolved per liter of solution.

Formula used :

where,

n = moles of solute = 5 moles

= volume of solution in liter  = ?

Therefore, the volume of solution in Liters is 2.22.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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