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mrs_skeptik [129]
3 years ago
9

What is the pressure of 1.20 moles of SO2 gas in a 4L container at 30 degrees celsius

Chemistry
2 answers:
geniusboy [140]3 years ago
6 0
Let suppose the Gas is acting Ideally, Then According to Ideal Gas Equation,

                                       P V  =  n R T
Solving for P,
                                       P  =  n R T / V     ----- (1)
Data Given;

Moles  = n = 1.20 mol

Volume  = V =  4 L

Temperature  = T = 30 + 273 = 303 K

Gas Constant  = R = 0.08206 atm.L.mol⁻¹.K⁻¹

Putting Values in Eq.1,

                     P  =  (1.20 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 303 K) ÷ 4 L

                     P  =  7.45 atm
sattari [20]3 years ago
3 0

Answer:

7.45 atm

Explanation:

Let suppose the Gas is acting Ideally, Then According to Ideal Gas Equation,

                                      P V  =  n R T

Solving for P,

                                      P  =  n R T / V     ----- (1)

Data Given;

Moles  = n = 1.20 mol

Volume  = V =  4 L

Temperature  = T = 30 + 273 = 303 K

Gas Constant  = R = 0.08206 atm.L.mol⁻¹.K⁻¹

Putting Values in Eq.1,

                    P  =  (1.20 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 303 K) ÷ 4 L

                    P  =  7.45 atm

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How many grams of F2 gas are there in a 5.00-L cylinder at 4.00 × 10^3 mm Hg and 23°C?
GuDViN [60]

Answer:

41.17g

Explanation:

We are given the following parameters for Flourine gas(F2).

Volume = 5.00L

Pressure = 4.00× 10³mmHG

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The formula we would be applying is Ideal gas law

PV = nRT

Step 1

We find the number of moles of Flourine gas present.

T = 23°C

Converting to Kelvin

= °C + 273k

= 23°C + 273k

= 296k

V = Volume = 5.00L

R = 0.08206L.atm/mol.K

P = Pressure (in atm)

In the question, the pressure is given as 4.00 × 10³mmHg

Converting to atm(atmosphere)

1 mmHg = 0.00131579atm

4.00 × 10³ =

Cross Multiply

4.00 × 10³ × 0.00131579atm

= 5.263159 atm

The formula for number of moles =

n = PV/RT

n = 5.263159 atm × 5.00L/0.08206L.atm/mol.K × 296K

n = 1.0834112811moles

Step 2

We calculate the mass of Flourine gas

The molar mass of Flourine gas =

F2 = 19 × 2

= 38 g/mol

Mass of Flourine gas = Molar mass of Flourine gas × No of moles

Mass = 38g/mol × 1.0834112811moles

41.169628682grams

Approximately = 41.17 grams.

3 0
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How many total atoms are in C3H-NO3?
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Answer:

Percent composition by element

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At standard ambient temperature and pressure (SATP), a gas has density of 1.5328g/L. What is the molar mass of the gas?
ahrayia [7]

The standard ambient temperature and pressure are

Temperature =298 K

Pressure = 1atm

The density of gas is 1.5328 g/L

density = mass of gas per unit volume

the ideal gas equation is

PV = nRT

P = pressure = 1 atm

V = volume

n = moles

R= gas constant = 0.0821 Latm/mol K

T = 298 K

moles = mass / molar mass

so we can write

n/V = density / molar mass

Putting values

Pressure=\frac{nRT}{V}=\frac{massXRT}{VXmolarmass}

Pressure=\frac{densityXRT}{molarmass}

molarmass=\frac{densityXRT}{Pressure}=\frac{1.5328X0.0821X298}{1}=37.50

Thus molar mass of gas is 37.50g/mol

6 0
3 years ago
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earnstyle [38]

Answer:

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Explanation:

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7 0
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