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sladkih [1.3K]
3 years ago
5

Suppose you are provided with a 30.86 g sample of potassium chlorate to perform this experiment. What is the mass of oxygen you

expect
to release upon heating?
Chemistry
1 answer:
oee [108]3 years ago
6 0

Answer:

The mass of oxygen is 12.10 g.

Explanation:

The decomposition reaction of potassium chlorate is the following:

2KClO₃(s) → 2KCl(s) + 3O₂(g)

We need to find the number of moles of KClO₃:

\eta_{KClO_{3}} = \frac{m}{M}

Where:

m: is the mass = 30.86 g

M: is the molar mass = 122.55 g/mol

\eta_{KClO_{3}} = \frac{30.86 g}{122.55 g/mol} = 0.252 moles                                      

Now, we can find the number of moles of O₂ knowing that the ratio between KClO₃ and O₂ is 2:3

\eta_{O_{2}} = \frac{3}{2}*0.252 moles = 0.378 moles

Finally, the mass of O₂ is:

m = 0.378 moles*32 g/mol = 12.10 g

Therefore, the mass of oxygen is 12.10 g.

I hope it helps you!

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Calculate the concentration of OH-in a solution that has a concentration of H+ = 8.1 x 10^−6 M at 25°C. Multiply the answer you
Nat2105 [25]

Answer:

The answer is 12.35

Explanation:

From the question we are given that the concentration of H^{+} is 8.1 * 18^{-6}M

 Generally The rate equation is given as

                                                           K_{w} = [H^{+} ][OH^{-} ]

and K_{w} the rate constant has a value 1 * 10^{-14}

     Substituting and making [OH^{-}] the subject we have

                                                 [OH^{-} ] = \frac{1 * 10^{-14}}{[H^{+}]} = \frac{1 * 10^{-14}}{8.1 *10^{-6}} =1.235 * 10^{-9}

                                                  [OH ^ {-}] = 1.235 * 10^{-9}M

                            Multiply the value by 10^{10} as instructed from the question we have  

                       Answer =   1.235 * 10 ^{-9} * 10^{10} = 12.35

Hence the answer in 2 decimal places is 12.35

7 0
3 years ago
A gas at 928 kpa, 129 C occupies a volume of 569 L. Calculate the volume at 319 kpa and<br> 32 C.
lisabon 2012 [21]

Answer:

1255.4L

Explanation:

Given parameters:

P₁  = 928kpa

T₁  = 129°C

V₁  = 569L

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T₂  = 32°C

Unknown:

V₂  = ?

Solution:

The combined gas law application to this problem can help us solve it. It is mathematically expressed as;

           \frac{P_{1} V_{1} }{T_{1} }   = \frac{P_{2} V_{2} }{T_{2} }

P, V and T are pressure, volume and temperature

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Now,

 take the units to the appropriate ones;

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P₂ = 319kpa in atm gives 3.15atm

P₁  = 928kpa gives 9.16atm

T₂  = 32°C gives 273 + 32  = 305K

T₁  = 129°C gives 129 + 273  = 402K

Input the values in the equation and solve for V₂;

        \frac{9.16  x 569}{402}   = \frac{3.15 x V_{2} }{305}

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