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1 year ago

Describe the relationship between volume and temperature of an ideal gas

Chemistry

1 answer:

kvv77 [185]1 year ago

8 0

Answer:

Explanation:

Here, we want to describe the relationship between the volume and temperature of an ideal gas

This relationship is defined by Charles' law

From this law, we know that the volume of a given mass of gas is directly proportional to its temperature at a fixed pressure

What this means is that as long as the pressure remains unchanged, when the volume increases, the temperature increases, and when the volume decreases, the temperature decreases

These can be represented by the mathematical formula below:

$\frac{V_1}{T_1}\text{ = }\frac{V_2}{T_2}$

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Answer:

Increases in temperature tend to decrease density since volume will generally increase. There are exceptions however, such as water's density increasing between 0°C and 4°C. Below is a table of units in which density is commonly expressed, as well as the densities of some common materials.

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3 years ago

Consider the equations below. (1) Fe2O3(s) → 2Fe(s) + 3 2 O2(g) (2) Fe2O3(s) + 3CO(g) → 2Fe(s)+3CO2(g) Which equation must be ad

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Answer:

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3 years ago

The heat capacity of an object depends on its ______

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Answer:

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Explanation:

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2 years ago

How many Zn atoms are there in 4.65 moles of Zn?

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3 years ago

The density of nitric oxide (NO) gas at 0.866 atm and 46.2 degrees celcius is ____ g/L

Artyom0805 [142]

Answer:

d = 0.992 g/L

Explanation:

Data Given:

Pressure of nitric oxide (NO) = 0.866 atm

Temperature of a gas = 46.2° C

Convert the temperature to kelvin = 46.2° C + 273

temperature in kelvin = 319.2 K

density of nitric oxide (NO) = ?

Solution:

Density of a gas can be calculated by

d = PM /RT

Where

d = density

P = Pressure

M = molar mass of gas

R = ideal gas constant = 0.0821 L atm mol⁻¹ K⁻¹

T = temperature

So,

Molar mass of NO = 30 g/mol

Put values in the formula:

d = PM /RT

d = 0.866 atm × 30 g/mol / 0.0821 L atm mol⁻¹ K⁻¹ × 319.2 K

d = 25.98 atm. g/mol / 26.2 L atm mol⁻¹

d = 0.992 g/L

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3 years ago