Question

What pressure (in atm) will 0.67 moles of C2H6(g)
have at 21.0 °C in a 500.0 mL container?

Answer 1

At 21.0 °C, 0.67 moles of
`C_2H_6(g)` in a 500.0 mL container exert a pressure of approximately 8.14 atm.

To find the pressure of a gas using the ideal gas law, you can use the formula:

PV = nRT

Where:

P is the pressure of the gas,

V is the volume of the gas,

n is the number of moles of the gas,

R is the ideal gas constant (0.0821 L·atm/(mol·K)),

T is the temperature in Kelvin.

First, convert the temperature from Celsius to Kelvin:

T(K) = T(°C) + 273.15

T = 21.0 + 273.15 = 294.15 K

Now, rearrange the ideal gas law to solve for pressure:

P = (nRT)/V

Plug in the values:

P = (0.67 mol)(0.0821 L·atm/(mol·K))(294.15 K) / 0.500 L

P ≈ 8.14 atm

So, the pressure of 0.67 moles of
`C_2H_6(g)` in a 500.0 mL container at 21.0 °C is approximately 8.14 atm.