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3 years ago

If 2 different gases have the same volumes but different masses, how will their densities compare?

Chemistry

2 answers:

Oxana [17]3 years ago

8 0

<h2>Answer:</h2>

<u>The gas having </u><u>greater mass will have greater density</u>

<h2>Explanation:</h2>

According to the equation of density

Density = $\frac{Mass}{Volume\\}$

We see that mass and density are directly proportional to each other if volume is constant

So the gas having greater mass will have greater density

olga_2 [115]3 years ago

3 0

can i have brainiest

The two samples will have the same density because they are the same substance. The volume will have increased just enough to balance the greater mass. Key Concept- When substances have the same volumes but different masses, the substance having the greatest mass will be the most dense.

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Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical

julia-pushkina [17]

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43.0 kJ

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The free energy (ΔG) measures the total energy that is presented in a thermodynamic system that is available to produce useful work, especially at thermal machines. In a reaction, the value of the variation of it indicates if the process is spontaneous or nonspontaneous because the free energy intends to decrease, so, if ΔG < 0, the reaction is spontaneous.

The standard value is measured at 25°C, 298 K, and the value of free energy varies with the temperature. It can be calculated by the standard-free energy of formation (G°f), and will be:

ΔG = ∑n*G°f products - ∑n*G°f reactants, where n is the coefficient of the substance in the balanced reaction.

By the balanced reaction given:

2NOCl(g) --> 2NO(g) + Cl2(g)

At ALEKS Data tab:

G°f, NOCl(g) = 66.1 kJ/mol

G°f, NO(g) = 87.6 kJ/mol

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3 years ago

A large balloon contains 5400 m3 of He gas that is kept at a temperature of 280 K and an absolute pressure of 1.10 x 105 Pa. Fin

patriot [66]

Answer:

1.02 × 10⁶ g

Explanation:

Step 1: Given data

Volume of the balloon (V): 5400 m³

Temperature (T): 280 K

Absolute pressure (P): 1.10 × 10⁵ Pa

Molar mass of He (M): 4.002 g/mol

Step 2: Convert "V" to L

We will use the conversion factor 1 m³ = 1000 L.

5400 m³ × 1000 L/1 m³ = 5.400 × 10⁶ L

Step 3: Convert "P" to atm

We will use the conversion factor 1 atm = 101325 Pa.

1.10 × 10⁵ Pa × 1 atm / 101325 Pa = 1.09 atm

Step 4: Calculate the moles of He (n)

We will use the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.09 atm × 5.400 × 10⁶ L / 0.08206 atm.L/mol.K × 280 K

n = 2.56 × 10⁵ mol

Step 5: Calculate the mass of He (m)

We will use the following expression.

m = n × M

m = 2.56 × 10⁵ mol × 4.002 g/mol

m = 1.02 × 10⁶ g

8 0

3 years ago