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2 years ago

Find gas pressure of 2.5 moles H2 and 4.6 moles Ne at 1400mmHg.

Chemistry

1 answer:

Monica [59]2 years ago

5 0

Answer:

Pressure of neon = 1.17 atm

Pressure of hydrogen = 0.63 atm

Explanation:

Given data:

Number of moles of H₂ = 2.5 mol

Number of moles of Ne = 4.6 mol

Total pressure = 1400 mmHg (1400/760 = 1.8 atm)

Solution:

We will solve this problem through mole fraction method.

Total number of moles = 2.5 + 4.6 = 7.1

Mole fraction of H₂ Mole fraction of Ne

2.5 mol/7.1 mol= 0.35 4.6mol/7.1mol = 0.65

Pressure of hydrogen = 0.35 × 1.8 atm

Pressure of hydrogen = 0.63 atm

Pressure of neon = 0.65 × 1.8 atm

Pressure of neon = 1.17 atm

Total pressure which is already given is sum of partial pressure of hydrogen and neon gas.

0.63 atm + 1.17 atm = 1.8 atm

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The balanced equation below shows the products that are formed when butane (C4H10) is combusted.

Nataly [62]

Answer:

2:8

Explanation:

The reaction equation is a given as:

2C₄H₁₀ + 130₂ → 8CO₂ + 10H₂O

From the reaction equation, the mole ratio is 2:8

Butane is C₄H₁₀

Carbon dioxide CO₂

From the reaction;

2 moles of butane will produce 8 moles of carbon dioxide

3 0

3 years ago

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How many grams of water are produced when 4.50 L of

MA_775_DIABLO [31]

The answer for the following problem has been mentioned below.

Therefore the mass of the water is 5.802 grams.

Explanation:

Given:

volume of oxygen (V) = 4.50 L

Temperature (T) = 425 K

pressure of oxygen (P) = 2.50 atm

Gram molecular mass of oxygen (M) = 16.0 grams

To calculate:

mass of water (m)

We know;

According to the ideal gas equation;

P × V = n × R × T

As we know;

no of moles = $\frac{m}{M}$

m represents the mass of oxygen (m)

M represents the Gram molecular mass (M)

According to above mentioned equation;

P × V = n × R × T

P represents the pressure of the oxygen

V represents the volume of the oxygen

n represents the no of moles of the oxygen

R represents the universal gas constant

where,

the value of R is 0.0821 L atm/K moles

Substituting the values in the above equation;

2.50 × 4.50 = $\frac{m}{16.0}$ × 0.0821 × 425

11.25 = $\frac{m}{16.0}$ × 34.8925

180 = m × 34.8925

m = $\frac{180}{34.8925}$

m = 5.158 grams

Therefore the mass of the of oxygen is 5.158 grams

Now;

As we know;

$\frac{m_{1} }{M_{1} } = \frac{m_{2} }{M_{2} }$

where;

$m_{1}$ represents the mass of the oxygen

$M_{1}$ represents the gram molecular mass of the oxygen

$m_{2}$ represents the mass of the water

$M_{2}$ represents the gram molecular mass of water

From the above given formula,

$\frac{5.158}{16.0}$ = $\frac{m_{2} }{18}$

where;

Gram molecular weight of water = 18.0 u

$m_{2}$ = 5.802 grams

Therefore the mass of the water is 5.802 grams.

5 0

3 years ago

A sample of methane gas, CH4, occupies 3.25 L at temperature of 19.0 o C. If the pressure is held constant, what will be the tem

Artemon [7]

Answer:

625.46 °C

Explanation:

We'll begin by converting 19 °C to Kelvin temperature. This can be obtained as follow:

T(K) = T(°C) + 273

T(°C) = 19 °C

T(K) = 19 °C + 273

T(K) = 292 K

Next, we shall determine the Final temperature. This can be obtained as follow:

Initial volume (V₁) = 3.25 L

Initial temperature (T₁) = 292 K

Final volume (V₂) = 10 L

Final temperature (T₂) =?

V₁/T₁ = V₂/T₂

3.25 / 292 = 10 / T₂

Cross multiply

3.25 × T₂ = 292 × 10

3.25 × T₂ = 2920

Divide both side by 3.25

T₂ = 2920 / 3.25

T₂ = 898.46 K

Finally, we shall convert 898.46 K to celsius temperature. This can be obtained as follow:

T(°C) = T(K) – 273

T(K) = 898.46 K

T(°C) = 898.46 – 273

T(°C) = 625.46 °C

Therefore the final temperature of the gas is 625.46 °C

4 0

3 years ago

The material the start all reactions are ______ and the materials that are formed are called _____.

max2010maxim [7]

Answer:

I think the second space is chemical bonds

7 0

3 years ago

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A flask holds 3.01 x 1023 molecules of carbon dioxide. The container is holding ________

sammy [17]

(B), because 1.0 moles would be 6.02 x 10^23 molecules. So you have half a mole.

8 0

3 years ago