A gas expands from 2.5 L to 8.6 L at a constant temperature. If the initial pressure is 1.6 atm, what is the final pressure?

Kazeer [188]

The symbol for hydrogen is H

3 0

3 years ago

At 1000 K, a sample of pure NO2 gas decomposes. 2 NO2(g) equilibrium reaction arrow 2 NO(g) + O2(g) The equilibrium constant KP

kirill115 [55]

<u>Answer:</u> The pressure of NO and $NO_2$ in the mixture is 0.58 atm and 0.024 atm respectively.

<u>Explanation:</u>

We are given:

Equilibrium partial pressure of $O_2$ = 0.29 atm

For the given chemical equation:

$2NO_2(g)\rightleftharpoons 2NO(g)+O_2(g)$

Initial: a

At eqllm: a-2x 2x x

Calculating for the value of 'x'

$\Rightarrow x=0.29$

Equilibrium partial pressure of NO = 2x = 2(0.29) = 0.58 atm

Equilibrium partial pressure of $NO_2$ = a - 2x = a - 2(0.29) = a - 0.58

The expression of $K_p$ for above equation follows:

$K_p=\frac{p_{O_2}\times (p_{NO})^2}{(p_{NO_2})^2}$

We are given:

$K_p=158$

Putting values in above expression, we get:

$158=\frac{0.29\times (0.58)^2}{(a-0.58)^2}\\\\a=0.555,0.604$

Neglecting the value of a = 0.555 because it cannot be less than the equilibrium concentration.

So, $a=0.604$

Equilibrium partial pressure of $NO_2$ = (a - 0.58) = (0.604 - 0.58) = 0.024 atm

Hence, the pressure of NO and $NO_2$ in the mixture is 0.58 atm and 0.024 atm respectively.

4 0

3 years ago

how much alum product would be lost to the crystallization solution if you had 42.5 ml of solution after filtration and the solu

JulsSmile [24]

Answer:

Total amount of alum lost = 0.5122 grams

Explanation:

Let the total volume of the solution be 100 mL

In 100 mL of solution, there is 2.63 gram of alum.

Out of this 100 mL solution, 42.5 mL is remaining.

Amount of alum in 42.5 mL solution is

$\frac{42.5}{100} * 2.63 = 1.117\\$ grams

Now the amount of alum lost is $2.63 -1.117 = 0.5122$ grams

3 0

3 years ago

1. If you have 8.1 g CO₂ and 2.3 g H₂, which one is the limiting reactant. Show your work. 2. Calculate the theoretical yield of

ZanzabumX [31]

Answer:

2.95 g of CH₄

Explanation:

To start this, we determine the equation:

4H₂ + CO₂ → CH₄ + 2H₂O

4 moles of hydrogen react to 1 mol of carbon dioxide in order to produce 1 mol of methane and 2 moles of water.

To determine the limiting reactant, we need to know the moles of each reactant.

8.1 g . 1 mol/ 44g = 0.184 moles of carbon dioxide

2.3 g . 1mol / 2g = 1.15 moles of hydrogen

4 moles of hydrogen react to 1 mol of CO₂

Then, 1.15 moles may react to (1.15 . 1) /4 = 0.2875 moles

We only have 0.184 moles of CO₂, so this is the limiting reactant. Not enough CO₂ to complete the 0.2875 moles that are needed.

Ratio is 1:1. 1 mol of CO₂ produces 1 mol of methane

Then, 0.184 moles of CO₂ will produce 0.184 moles of CH₄

We convert moles to mass: 0.184 mol . 16 g /mol = 2.95 g

7 0

3 years ago

Which solution has the greatest number of hydroxide ions?baking soda, pH = 9milk, pH = 6tomato juice, pH = 3.5vinegar, pH = 2

weqwewe [10]

Answer: -

Baking soda having a pH of 9, has the maximum number of hydroxide ions.

Explanation: -

More the pH of a solution, the more basic it is and more the number of hydroxide ions it has.

From the question we find that

baking soda has a pH = 9

milk has a pH = 6

tomato juice has a pH = 3.5

vinegar has a pH = 2

Thus among them baking soda has the highest pH.

So baking soda is the most basic and has the maximum number of hydroxide ions.

8 0

4 years ago

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