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vazorg [7]
4 years ago
9

A 250.0-ml sample of ammonia, nh3 (g), exerts a pressure of 833 torr at 42.4 °c. what mass of ammonia is in the container

Chemistry
1 answer:
Lelu [443]4 years ago
6 0
To solve this, let's assume ideal gas behavior.

PV=nRT
Let's solve for n. Convert units to SI units first.

Pressure = 833 torr(101325 Pa/760 torr) = 111,057.53 Pa
Volume = 250 mL(1 L/1000 mL)(1 m³/1000 L) = 2.5×10⁻⁴ m³
Temperature = 42.4 + 273 = 315.4 K

n = (8,314 J/mol·K)(315.4 K)/(111057.53 Pa)(2.5×10⁻⁴ m³)
n = 94.45 mol

The molar mass of ammonia is 17.031 g/mol.
Mass = 94.45*17.031 = <em>1,608.51 g ammonia</em>


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<h3>Answer:</h3>

4551.37 Pascals

<h3>Explanation:</h3>

The pressure refers to the force exerted by a substance per unit area.

The pressure is liquid is calculated by;

P = height × density × gravitational acceleration

In this case;

Height = 636.2 mm

Density = 0.7300 g/cm³

g = 9.8 N/kg

We need to convert mm to m and g/cm³ to kg/m³

Therefore;

Height = 636.2 mm ÷1000

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Then, we can calculate the pressure;

Pressure = 0.6362 m × 730 kg/m³ × 9.8 N/kg

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               = 4551.37 Pascals

Therefore, the pressure of the column of decane is 4551.37 Pascals

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