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olchik [2.2K]
3 years ago
11

What is the mass of water necessary to generate 11.2 L of hydrogen gas if calcium metal reacts with water at standard temperatur

e and pressure (STP)?
Chemistry
1 answer:
12345 [234]3 years ago
5 0

Answer:

The mass of water is 18 g

Explanation:

The reaction of calcium with water can be represented in the equation below:

Ca + 2H₂O --------->Ca(OH)₂ +H₂

1 Mole of gas at STP = 22.4L

From the displacement reaction above, calculate the mass of water that will produce 22.4L of hydrogen gas at STP.

Mass of 2H₂O = 2(2x1 + 16) = 2X18 = 36 g/mol

Using proportional analysis;

36 g of 2H₂O produced 22.4 L of H₂, then

what mass of 2H₂O will produce 11.2L of  H₂ ?

Mathematically,

22.4 L ----------------------------------> 36g

11.2 L -----------------------------------> ?

Cross and multiply, to obtain the expression below

= (11.2 X 36)/22.4

= 18 g

Therefore, the mass of water is 18 g

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The equilibrium constant for the reaction AgBr(s) Picture Ag+(aq) + Br− (aq) is the solubility product constant, Ksp = 7.7 × 10−
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Answer:

The reaction will be  non spontaneous at these concentrations.

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\Delta G=40.588 kJ/mol

  • For reaction to spontaneous reaction:  \Delta G.
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Since ,the value of Gibbs free energy is greater than zero which means reaction will be non spontaneous at these concentrations

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