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1 year ago

How do I do this partial pressure problem? (AP CHEM)

Chemistry

1 answer:

RoseWind [281]1 year ago

7 0

The partial pressure of H(g) is 1.07 atm.

<h3>What is the partial pressure?</h3>

We know that the total pressure of a mixture of gases is the sum of the individual pressure of the gases. Now we know from the Dalton law of partial pressure that the total pressure PT = PA + PB + PC + ........

Thus, the molecular hydrogen has a pressure of 2.14 atm and this molecular hydrogen is made to decompose. The partial pressure of each of the H(g) is 2.14/2 = 1.07 atm.

Hence, the partial pressure of H(g) is 1.07 atm.

Learn more about partial pressure:brainly.com/question/13199169

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Which type of formula represents the simplest whole-number ratio of atoms of the elements in a compound?

sleet_krkn [62]

The empirical formula represents the simplest whole number shows the simplest whole number ratio of atoms in a compound. An example of this is the empirical formula for glucose (C₆H₁₂O₆) is C₃H₆O₃.

I hope this helps. Let me know if anything is unclear.

5 0

3 years ago

What is the temperature of 4.5 moles of a gas that occupies 50. mL at 1.35 atm?

devlian [24]

Answer:

$T = 0.182$ Kelvin

Explanation:

As we know that

$PV = nRT\\$

Where P is the pressure in atmospheric pressure

T is the temperature in Kelvin

R is the gas constant

V is the volume in liters

$R = 0.08206$

Substituting the given values in above equation, we get -

$1.35 * \frac{50}{1000}= 4.5 * 0.08206* T\\$

On rearranging, we get

$T = \frac{1.35*50}{1000*0.08206*4.5} \\$

$T = 0.182$ Kelvin

7 0

3 years ago

If the sample contained 2.0 moles of KClO3 at a temperature of 214.0 °C, determine the mass of the oxygen gas produced in grams

Westkost [7]

Answer : The mass of the oxygen gas produced in grams and the pressure exerted by the gas against the container walls is, 96 grams and 1.78 atm respectively.

Explanation : Given,

Moles of $KCl_3$ = 2.0 moles

Molar mass of $O_2$ = 32 g/mole

Now we have to calculate the moles of $MgO$

The balanced chemical reaction is,

$2KClO_3\rightarrow 2KCl+3O_2$

From the balanced reaction we conclude that

As, 2 mole of $KClO_3$ react to give 3 mole of $O_2$

So, 2.0 moles of $KClO_3$ react to give $\frac{2.0}{2}\times 3=3.0$ moles of $O_2$

Now we have to calculate the mass of $O_2$

$\text{ Mass of }O_2=\text{ Moles of }O_2\times \text{ Molar mass of }O_2$

$\text{ Mass of }O_2=(3.0moles)\times (32g/mole)=96g$

Therefore, the mass of oxygen gas produced is, 96 grams.

Now we have to determine the pressure exerted by the gas against the container walls.

Using ideal gas equation:

$PV=nRT\\\\PV=\frac{w}{M}RT\\\\P=\frac{w}{V}\times \frac{RT}{M}\\\\P=\rho\times \frac{RT}{M}$

where,

P = pressure of oxygen gas = ?

V = volume of oxygen gas

T = temperature of oxygen gas = $214.0^oC=273+214.0=487K$

R = gas constant = 0.0821 L.atm/mole.K

w = mass of oxygen gas

$\rho$ = density of oxygen gas = 1.429 g/L

M = molar mass of oxygen gas = 32 g/mole

Now put all the given values in the ideal gas equation, we get:

$P=1.429g/L\times \frac{(0.0821L.atm/mole.K)\times (487K)}{32g/mol}$

$P=1.78atm$

Thus, the pressure exerted by the gas against the container walls is, 1.78 atm.

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3 years ago

A. Clearly draw the Lewis structure for the PBr4- ion. Show your math where

Nataliya [291]

Answer:

Br-P-Br

Explanation:

To calculate the valance electrons, look at the periodic table to find the valance electrons for each atom and add them together. P is in column 5A, so it has 5, Br is in column 7A, so it has 7 (multiply by 4 since there are 4 Br atoms to give 28) and there is a 1- charge, so add one more electron. 5+28+1=34, so there are 34 electrons to place. P would be the central atom, so place it in the middle. Place each Br around the P (as shown above) with a a single line connecting it. Each line represents 2 electrons, so 8 total have been place, leaving 26 remaining. Place 6 electrons around each Br (2 on each of the unbonded sides), which leaves 2 electrons remaining. The remaining pair of unbound electrons will be attached to the P between any two Br atoms. Phosphorus doesn't have to follow the octet rule, so it actually ends up with 10 valance electrons.

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3 years ago

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How can you tell that a white powder is salt without tasting it?

ZanzabumX [31]

You can detect salt in water without tasting by measuring the density of the water. Place a glass of spring water and a glass of the suspected salt water on a balance scale and the heavier one contains salt. Other ways to test for salt in water is to put a drop of water on the end of a nail and place in a gas flame. If the water contains salt, the flame will turn a yellow/orange color.

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3 years ago