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ss7ja [257]
2 years ago
12

A gas phase mixture of H2 and N2 has a total pressure of 784 torr with an H2 partial pressure of 124 torr. What mass of N2 gas i

s present in 2.00 L of the mixture at 298 K
Chemistry
1 answer:
olchik [2.2K]2 years ago
4 0

The mass of N₂ in the mixture having a total pressure of 784 torr with an H₂ partial pressure of 124 torr is 1.988 g

We'll begin by calculating the partial pressure of N₂. This can be obtained as follow:

Total pressure = 784 torr

Partial pressure of H₂ = 124 torr

<h3>Partial pressure of N₂ =?</h3>

Total pressure = Partial pressure of H₂ + Partial pressure of N₂

784 = 124 + Partial pressure of N₂

Collect like terms

Partial pressure of N₂ = 784 – 124

<h3>Partial pressure of N₂ = 660 Torr</h3>

  • Next, we shall determine the number of mole of N₂ in the mixture.

Pressure of N₂ (P) = 660 Torr

Volume (V) = 2 L

Temperature (T) = 298 K

Gas constant (R) = 62.364 L.Torr/Kmol

<h3>Number of mole of N₂ (n) =? </h3>

PV = nRT

660 × 2 = n × 62.364 × 298

1320 = n × 18584.472

Divide both side by 18584.472

n = 1320 / 18584.472

<h3>n = 0.071 mole</h3>

  • Finally, we shall determine the mass of N₂ in the mixture.

Mole of N₂ = 0.071 mole

Molar mass of N₂ = 2 × 14 = 28 g/mol

<h3>Mass of N₂ =? </h3>

Mass = mole × molar mass

Mass of N₂ = 0.071 × 28

<h3>Mass of N₂ = 1.988 g</h3>

Therefore, the mass of N₂ in the mixture having a total pressure of 784 torr with an H₂ partial pressure of 124 torr is 1.988 g

Learn more: brainly.com/question/20853110

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When iridium-192 is used in cancer treatment, a small cylindrical piece of 192ir, 0.6 mm in diameter and 3.5 mm long, is surgica
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Iridium-192 is used in cancer treatment, a small cylindrical piece of 192 Ir, 0.6 mm in diameter (0.3mm radius) and 3.5 mm long, is surgically inserted into the tumor. if the density of iridium is 22.42 g/cm3, how many iridium atoms are present in the sample?

Let us start by computing for the volume of the cylinder. V = π(r^2)*h where r and h are the radius and height of the cylinder, respectively. Let's convert all given dimensions to cm first. Radius = 0.03 cm, height is 0.35cm long.

V = π * (0.03cm)^2 * 0.35 cm = 9.896*10^-4 cm^3

Now we have the volume of 192-Ir, let's use the density provided to get it's mass, and once we have the mass let's use the molar mass to get the amount of moles. After getting the amount of moles, we use Avogadro's number to convert moles into number of atoms. See the calculation below and see if all units "cancel":

9.896*10^-4 cm^3 * (22.42 g/cm3) * (1 mole / 191.963 g) * (6.022x10^23 atoms /mole)

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What happens to the rate of a reaction as the reaction progresses?
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Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0g of potassium and
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Answer:

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Explanation:

To adequately solve this problem, we should know the law of constant composition. This is a pointer to the fact that no matter the type of sample, the percentage compositions of potassium and iodine still remains the same. We can use these masses to get a formula and we would know the percentage compositions in whatever mass we are dealing with.

First of all, we add the masses in the first sample. 13 + 42.3 = 55.3

Hence, the percentage composition of the potassium is 13/55.3 * 100 = 23.51%

The percentage composition of the iodine is = 100 - 23.51 = 76.49%

Now, we need to get the formula of the compound. We can get this by dividing the percentage compositions with the atomic masses. The atomic mass of potassium and iodine is 39 and 127 respectively.

Potassium = 23.51/39 =0.603

Iodine = 76.49/127 = 0.602

We then divide by the smaller value to get the formula and this shoes our formula is KI

We can see they have a ratio of 1 to 1, meaning one atom of potassium to one atom of iodine. This further confirms the percentage compositions of 23.5 to 76.5

Now to get the mass of iodine yielded, let us say the mass is xkg

This means x/(x + 24.4) * 100 = 76.5

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100x - 76.5x = 1866.6

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