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MrRa [10]
3 years ago
14

What temperature would 3.54 moles of xenon gas need to reach to exert a pressure of 1.57 atm at a volume of 34.6 l

Chemistry
1 answer:
ira [324]3 years ago
5 0

Answer:

186.9Kelvin

Explanation:

The ideal gas law equation is PV = n R T

where

P   is the pressure of the gas

V   is the volume it occupies

n  is the number of moles of gas present in the sample

R  is the universal gas constant, equal to  0.0821 atm L /mol K

T  is the absolute temperature of the gas

Ensure units of the volume, pressure, and temperature of the gas correspond to R ( the universal gas constant, equal to  0.0821 atm L /mol K )

n = 3.54moles

P= 1.57

V= 34.6

T=?

PV = n R T

PV/nR = T

1.57 x 34.6/3.54 x 0.0821

54.322/0.290634= 186.908620464= T

186.9Kelvin ( approximately to 1 decimal place)

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The average Kenectic energy

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The ion MnOis often used to analyze for the Fe2+ content of an aqueous solution by using the (unbalanced) reaction Mno+Fe2+ + Fe
dusya [7]

Answer:

B) 0.230 M

Explanation:

The first step is to <u>balance the reaction</u> between the Ferrous ion and the permanganate ion:

5~Fe^+^2~+~MnO_4^-^1~+~8H^+~->~5Fe^+^3~+~Mn^+^2~+4H_2O

Then we have to <u>calculate the moles</u> of MnO_4^-:

M~=~\frac{mol}{L}

mol~=~M*L

mol~=~0.033~M*0.0633L=~0.002088~mol~MnO_4^-

Then using the <u>molar ratio</u> we can find the moles of Fe^+^2:

0.002088~mol~MnO_4^-\frac{5~mol~Fe^+^2}{1~mol~MnO_4^-}=0.01044~mol~Fe^+^2

Finally we can calculate the molarity:

M=\frac{0.01044~mol~Fe^+^2}{0.0455~L}=0.230~M

5 0
3 years ago
Name the organic compound of ch3chohch2ch3
snow_lady [41]

Answer:

Flavouring agent 2-Butanol, or sec-butanol, is an organic compound with formula CH3CH(OH)CH2CH3.

4 0
2 years ago
A student titrates 10.00 milliliters of hydrochloric acid of unknown molarity with 1.000 m naoh. it takes 21.17 milliliters of b
Dima020 [189]
Mole ratio for the reaction is 1:1
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4 0
3 years ago
When sulfur burns in air, it forms sulfur dioxide as shown by the equation below.what volume of SO2 is produced when 2.35 g of s
Naddik [55]

1.64 L of sulfur dioxide (SO₂)

Explanation:

We have the following chemical reaction:

S (s) + O₂ (g) → SO₂ (g)

First we calculate the number of moles of sulfur (S):

number of moles = mass / molar weight

number of moles of sulfur = 2.35 / 32 = 0.0734 moles

Looking at the chemical reaction we see that 1 moles of sulfur (S) produces 1 moles of sulfur dioxide (SO₂), so 0.0734 moles of sulfur will produce 0.0734 moles of sulfur dioxide (SO₂).

To calculate the volume of sulfur dioxide (SO₂), assuming that the sulfur dioxide is behaving as an ideal gas and the we determine the gas volume under standard temperature and pressure conditions, we use the following formula:

number of moles = volume / 22.4 (L/mole)

volume = number of moles × 22.4

volume of SO₂ = 0.0734 × 22.4 = 1.64 L

Learn more about:

molar volume

brainly.com/question/11160940

brainly.com/question/506048

#learnwithBrainly

PS: I appreciate that you took the time and effort to write the chemical equation in a readable way. This makes the question to be very rare :D

5 0
3 years ago
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