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GarryVolchara [31]
3 years ago
8

If the sample contained 2.0 moles of KClO3 at a temperature of 214.0 °C, determine the mass of the oxygen gas produced in grams

and the pressure exerted by the gas against the container walls.
Chemistry
1 answer:
Westkost [7]3 years ago
7 0

Answer : The mass of the oxygen gas produced in grams and the pressure exerted by the gas against the container walls is, 96 grams and 1.78 atm respectively.

Explanation : Given,

Moles of KCl_3 = 2.0 moles

Molar mass of O_2 = 32 g/mole

Now we have to calculate the moles of MgO

The balanced chemical reaction is,

2KClO_3\rightarrow 2KCl+3O_2

From the balanced reaction we conclude that

As, 2 mole of KClO_3 react to give 3 mole of O_2

So, 2.0 moles of KClO_3 react to give \frac{2.0}{2}\times 3=3.0 moles of O_2

Now we have to calculate the mass of O_2

\text{ Mass of }O_2=\text{ Moles of }O_2\times \text{ Molar mass of }O_2

\text{ Mass of }O_2=(3.0moles)\times (32g/mole)=96g

Therefore, the mass of oxygen gas produced is, 96 grams.

Now we have to determine the pressure exerted by the gas against the container walls.

Using ideal gas equation:

PV=nRT\\\\PV=\frac{w}{M}RT\\\\P=\frac{w}{V}\times \frac{RT}{M}\\\\P=\rho\times \frac{RT}{M}

where,

P = pressure of oxygen gas = ?

V = volume of oxygen gas

T = temperature of oxygen gas = 214.0^oC=273+214.0=487K

R = gas constant = 0.0821 L.atm/mole.K

w = mass of oxygen gas

\rho = density of oxygen gas = 1.429 g/L

M = molar mass of oxygen gas = 32 g/mole

Now put all the given values in the ideal gas equation, we get:

P=1.429g/L\times \frac{(0.0821L.atm/mole.K)\times (487K)}{32g/mol}

P=1.78atm

Thus, the pressure exerted by the gas against the container walls is, 1.78 atm.

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Complete Question

Magnesium sulfate forms a hydrate with the formula MgSO_4. 7H_20. What is the maximum amount of water (in grams) that can be removed from 15 ml of toluene by the addition of 200 mg of anhydrous magnesium sulfate? The molar mass of MgSO_4 is 120.4 g/mol; H20 = 18 g/mol.

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Explanation:

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   The volume of toluene is  V = 15 mL

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   The formula of the hydrate is   MgSO_4. 7H_20

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From the formula given we see that

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Hence

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  1 g of Mg SO_4 will remove  x  =  1.0465 \  g  of  H_2O  

Then  

   200 *10^{-3} \  g of Mg SO_4 will remove z g of  x  =  1.0465 \  g  of  H_2O  

So

   z =  200 *10^{-3} *  1.0465

=>z =  200 *10^{-3} *  1.0465

=>z =  0.2093 \  g of  H_2O  

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