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Over [174]
2 years ago
7

In the lab, a 156 g sample of unknown compound KClOx was completely decomposed to produce 50.4 L of O2 (g) at STP and an unknown

amount of KCl. What is the value of X
Chemistry
1 answer:
aleksandr82 [10.1K]2 years ago
6 0

Answer:

2

Explanation:

Step 1: Write the generic decomposition reaction

KClOₓ ⇒ KCl + O₂

Step 2: Calculate the moles of O₂

At STP, 1 mole of an ideal gas occupies 22.4 L.

50.4 L × 1 mol/22.4 L = 2.25 mol

Step 3: Calculate the mass corresponding to 2.25 moles of O₂

The molar mass of O₂ is 32.00 g/mol.

2.25 mol × 32.00 g/mol = 72 g

Step 4: Determine the value of x

Every 156 g of KClOₓ there are 72 g of oxygen. The mass percent of O is:

%O: 72 g/156 g × 100% = 46.2%

In KClO, the mass percent of O is: 32.00 g/90.5 g × 100% = 35.4%

In KClO₂, the mass percent of O is: 64.00 g/138.5 g × 100% = 46.2%

Then, x = 2

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Like several other bonds, carbon-oxygen bonds have lengths and strengths that depend on the bond order. Draw Lewis structures fo
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<h3>What is bond length?</h3>

The distance between the centers of two atoms that are covalently connected is known as the bond length. The number of bound electrons determines the bond's length (the bond order). The greater the attraction between the two atoms and the shorter the bond length are, the higher the bond order.

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5 0
1 year ago
Ammonia is formed according to the reaction below. A chemist mixes 21 grams of nitrogen gas and 18 grams of hydrogen gas in a 2.
Rama09 [41]

Answer : The mass of hydrogen gas consumed will be, 4.5 grams

Explanation : Given,

Mass of N_2 = 21 g

Mass of H_2 = 18 g

Molar mass of N_2 = 28 g/mole

Molar mass of H_2 = 2 g/mole

First we have to calculate the moles of N_2 and H_2.

\text{Moles of }N_2=\frac{\text{Mass of }N_2}{\text{Molar mass of }N_2}=\frac{21g}{28g/mole}=0.75moles

\text{Moles of }H_2=\frac{\text{Mass of }H_2}{\text{Molar mass of }H_2}=\frac{18g}{2g/mole}=9moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

N_2(g)+3H_2(g)\rightarrow 2NH_3(g)

From the given balanced reaction, we conclude that

As, 1 mole of N_2 react with 3 moles of H_2

So, 0.75 moles of N_2 react with 3\times 0.75=2.25 moles of H_2

From this we conclude that, H_2 is an excess reagent because the given moles are greater than the required moles and N_2 is a limiting reagent because it limits the formation of product.

The moles of hydrogen gas consumed = 2.25 mole

Now we have to calculate the mass of hydrogen gas consumed.

\text{Mass of }H_2=\text{Moles of }H_2\times \text{Molar mass of }H_2

\text{Mass of }H_2=(2.25mole)\times (2g/mole)=4.5g

Therefore, the mass of hydrogen gas consumed will be, 4.5 grams

5 0
3 years ago
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