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nordsb [41]
3 years ago
8

A certain gas at 2oC and 1.00 atm pressure fills a 4.0 container. What volume will the gas occupy at 100oC and 780 torr pressure

?
Chemistry
1 answer:
artcher [175]3 years ago
6 0

The final volume V₂=4.962 L

<h3>Further explanation</h3>

Given

T₁=20 + 273 = 293 K

P₁= 1 atm

V₁ = 4 L

T₂=100+273 = 373 K

P₂=780 torr=1,02632 atm

Required

The final volume

Solution

Combined gas law :

P₁V₁/T₁=P₂V₂/T₂

Input the value :

V₂=(P₁V₁T₂)/(P₂T₁)

V₂=(1 x 4 x 373)/(1.02632 x 293)

V₂=4.962 L

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Answer:

The electron geometry, molecular geometry and idealized bond angles for these molecules respectively are:

a. CF4: tetrahedral, tetrahedral and 109.5 degrees

b. NF3 tetrahedral, trigonal pyramidal and 102.5 degrees

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d. H2S tetrahedral, angular and 92.1 degrees

Explanation:

The electron geometry considers the bound atoms and unbound electron pairs to determine the geometry. The four molecules have four bound atoms and/or unbound electrons pairs, thus they have a tetrahedral geometry. On the other hand, the molecular geometry only considers the position of bound atoms to determine the geometry.

Between H3O and H2O, H2O has a smaller bond angle due to the two unbound electron pairs. The bond angle decrease as the number of unbound electron pairs increases in every molecule.

CO2 and CCl4 are both nonpolar because of the 3D geometry of the molecule. Each individual bond is polar but both molecules have symmetrical geometry so the dipole bonds are canceled.

CH3F  is a polar molecule because the dipole between the C-H and C-F bonds are differents thus, besides the symmetrical geometry the dipole bonds are not canceled.

8 0
3 years ago
If .00327 g of a gas dissolves in 0.376 L of water at 867 torr, what quantity of this gas (in grams) will dissolve at 759 torr?
Vinil7 [7]

At 759 torr, 0.002 86 g of the gas will dissolve.

Henry’s law states:

c = k_{H}p, where

where K_{H} is a proportionality constant called the Henry's Law constant.

If we have the same solute in the same solvent at two different pressures  p_{1} and p_{2},  

c_{1} = k_{H}p_{1} and c_{2} = k_{H}p_{2}

Dividing the two equations, k_H cancels and we get

c_1/c_2 = p_1/p_2

<em>c</em>_2 = <em>c</em>_1 × <em>p</em>_2/<em>p</em>_1

The volumes of solvent are the same, so we can use the masses of the solute instead of concentrations.

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What is the maximum number of grams of PH3 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH3
kvv77 [185]

Answer:

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Ratio is 2:2. So 2 moles of P can produce 2 moles of phosphine. Therefore, 0.2 moles of P must produce the same amount of phosphine.

Let's convert the moles to mass ( mol . molar mass)

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