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yawa3891 [41]
3 years ago
14

What is the molar concentration (molarity) of 1.0 mol of KCl dissolved in 750 mL of

Chemistry
1 answer:
Nikolay [14]3 years ago
8 0

Answer:

Molarity is moles per liter. You have one mole in 0.750 liters

Explanation:

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Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25
o-na [289]
The equation Eºcell = 0.0592/n logK must be used to find n and also Eºcell 
2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s) Al3+ +3e- --> Al Eº = -1.66 V Mg2+ +2e- -->Mg Eº = -2.37V 
To balance the equation, 6 moles of electrons must be transferred (2 Al and 3 Mg). This will be the value of n in the equation. 
To find Eºcell, you need the reduction potentials which should be given in a table, and given above. Eºcell = -1.66 - (-2.37) = 0.71 V log K = Eºcell x n/0.0592 = 0.71 x 6/0.0592 log K = 71.95 K = 10^71.95 K = 1.1x10^72
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Legumes are much easier to grow than other plants, and are more adaptable.

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Sitting at a four-legged table there is: 1 grandma, 2 moms, 2 daughters and a granddaughter. How many legs are under the table?
lbvjy [14]

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The answer is 14 "legs"

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3 0
3 years ago
Iodine, I2, is a solid at room temperature but sublimes (converts from a solid into a gas) when warmed. What is the temperature
Stels [109]
<h3>Answer:</h3>

382.63 K

<h3>Explanation:</h3>

We are given;

  • Volume of Iodine as 71.4 mL
  • Mass of Iodine as 0.276 g
  • Pressure of Iodine as 0.478 atm

We are required to calculate the temperature of Iodine

  • We are going to use the ideal gas equation;
  • According to the ideal gas equation; PV = nRT, where R is the ideal gas constant, 0.082057 L.atm/mol.K.
  • Rearranging the formula;

T = PV ÷ nR

But, n, the number of moles = Mass ÷ Molar mass

Molar mass of iodine = 253.8089 g/mol

Thus, n = 0.276 g ÷ 253.8089 g/mol

           = 0.001087 moles

Therefore;

T = (0.478 atm × 0.0714 L) ÷ (0.001087 moles × 0.082057)

  = 382.63 K

Thus, the temperature of Iodine in Kelvin is 382.63 K

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3 years ago
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