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trasher [3.6K]
3 years ago
12

A rigid tank contains 0.66 mol of oxygen (O2). Find the mass of oxygen that must be withdrawn from the tank to lower the pressur

e of the gas from 43 atm to 17 atm. Assume that the volume of the tank and the temperature of the oxygen are constant during this operation. Answer in units of g.
Chemistry
1 answer:
dsp733 years ago
7 0

Answer:

12.8 g of O_{2} must be withdrawn from tank

Explanation:

Let's assume O_{2} gas inside tank behaves ideally.

According to ideal gas equation- PV=nRT

where P is pressure of O_{2}, V is volume of O_{2}, n is number of moles of O_{2}, R is gas constant and T is temperature in kelvin scale.

We can also write, \frac{V}{RT}=\frac{n}{P}

Here V, T and R are constants.

So, \frac{n}{P} ratio will also be constant before and after removal of O_{2} from tank

Hence, \frac{n_{before}}{P_{before}}=\frac{n_{after}}{P_{after}}

Here, \frac{n_{before}}{P_{before}}=\frac{0.66mol}{43atm} and P_{after}=17atm

So, n_{after}=\frac{n_{before}}{P_{before}}\times P_{after}=\frac{0.66mol}{43atm}\times 17atm=0.26mol

So, moles of O_{2} must be withdrawn = (0.66 - 0.26) mol = 0.40 mol

Molar mass of O_{2} = 32 g/mol

So, mass of O_{2} must be withdrawn = (32\times 0.40)g=12.8g

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iron is made by a reduction of iron oxide with carbon monoxide. Fe2O3+3CO-2Fe+3CO2. Calculate the mass of iron that can be forme
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Mass = 88.12 g

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Mass of iron formed = ?

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Fe₂O₃ + 3CO    →      2Fe + 3CO₂

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Now we will compare the moles of iron with iron oxide.

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