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Vlad [161]
3 years ago
9

At what temperature will 2.40 moles of chlorine gas exert a pressure of 2.70 atm at a volume of 0.750 L?

Chemistry
2 answers:
Kamila [148]3 years ago
8 0

Answer:

—262.71°C

Explanation:

Step 1:

The following data were obtained from the question:

Number of mole (n) = 2.4 moles

Pressure (P) = 2.70 atm

Volume (V) = 0.750 L

Temperature (T) =?

Gas constant (R) = 0.082atm.L/Kmol

Step 2:

Determination of the temperature.

Using the ideal gas equation, the temperature can be obtained as follow:

PV = nRT

2.7 x 0.750 = 2.4 x 0.082 x T

Divide both side by 2.4 x 0.082

T = (2.7 x 0.750) /(2.4 x 0.082)

T = 10.29K

Step 3:

Conversion of Kelvin temperature to celsius temperature.

Temperature (celsius) = temperature (Kelvin) - 273

temperature (Kelvin) = 10.29K

Temperature (celsius) = 10.29 - 273

Temperature (celsius) = —262.71°C

DochEvi [55]3 years ago
6 0

Answer:

10.28Kelvin

Explanation:

Using the ideal gas equation;

PV = nRT

P is the pressure

V is the volume of the gas

n is the number of moles

T is the temperature in Kelvin

R is the Gas constant

Given n = 2.4moles

P = 2.70atm

V = 0.750L

R = 0.0821atm.L/mol.K

From the formula above:

T = PV/nR

T = 2.70×0.750/2.4×0.0821

T = 2.025/0.197

T = 10.28K

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4121 years

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7 0
3 years ago
How many moles are present in 54.8 mL of mercury if the density of mercury is 13.6 g/mL?​
lesya692 [45]

Answer:

3.72 mol Hg

General Formulas and Concepts:

<u>Chemistry - Atomic Structure</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis
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Explanation:

<u>Step 1: Define</u>

D = 13.6 g/mL

54.8 mL Hg

<u>Step 2: Identify Conversions</u>

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<u>Step 3: Find</u>

13.6 g/mL = x g / 54.8 mL

x = 745.28 g Hg

<u>Step 4: Convert</u>

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<em>We are given 3 sig figs. Follow sig fig rules and round.</em>

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