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pochemuha
3 years ago
7

How many grams of oxygen are required to produce

Chemistry
1 answer:
Likurg_2 [28]3 years ago
8 0

Answer:

8 GRAMS OF OXYGEN WILL BE REQUIRED TO PRODUCE 9 GRAMS OF WATER MOLECULES.

Explanation:

The equation for the reaction is;

2 H + O2 ----> 2 H2O          

(H = 1, O = 16)

From the reaction, it can be observed that 1 mole of O2 reacts to form 2 moles of H2O

At STP, using the molar masses of the elememts and compound in the reaction, 32 g of O2 will reacts to form 36 g (18 * 2 g) of H2O

32 g of O2 = 36 g OF H2O

if 9 grams of H2O is produced, the mass of oxygen required to produce it will be:

( 32 * 9 / 36 ) g of O2

= (288 / 36) g

= 8 g of O2

So, 8 grams of Oxygen will be required to produce 9 grams of water.

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An unknown gas effuses at one half the speed of oxygen. What is the molar mass of the unknown? It is either HBr or HI. Which gas
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Explanation:

  • Thomas Graham found that, at a constant  temperature and pressure the rates of effusion  of various gases are inversely proportional to  the square root of their masses.

Rate of effusion ∝ 1/√molar mass.

  • <em>(Rate of effusion of O₂) / (Rate of effusion of unknown gas) = (√molar mass of unknown gas) / (√molar mass of O₂).</em>
  • An unknown gas effuses at one half the speed of that of oxygen.

∵ Rate of effusion of unknown gas = 1/2 (Rate of effusion of O₂)

∴ (Rate of effusion of O₂) / (Rate of effusion of unknown gas) = 2.

Molar mass of O₂ = 32.0 g/mol.

∵ (Rate of effusion of O₂) / (Rate of effusion of unknown gas) = (√molar mass of unknown gas) / (√molar mass of O₂).

∴  2.0 = (√molar mass of unknown gas) / √32.0.

( √molar mass of unknown gas) = 2.0 x √32.0

By squaring the both sides:

∴ molar mass of unknown gas = (2.0 x √32.0)² = 128 g/mol.

∴ The molar mass of sulfur dioxide = 80.91 g/mol and the molar mass of HI = 127.911 g/mol.

<em>So, the unknown gas is HI.</em>

<em></em>

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