How would you find the volume of 7 moles of CH4 at standard temperature and pressure?

Question

How would you find the volume of 7 moles of CH4 at standard temperature and pressure?

1 Answer

Impact of this question

2004 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2015-11-13T07:33:20

The volume of 7 moles of ${CH}_{4}$ $"CH"_4"$ at STP is approximately $200 L$ $"200 L"$ .

Explanation:

STP is 273.15 K and 100 kPa.

Use the ideal gas law, $P V = n R T$ $PV=nRT$ , where $P$ $P$ is pressure, $V$ $V$ is volume, $n$ $n$ is moles, $R$ $R$ is the gas constant, and $T$ $T$ is temperature.

$P = 100 kPa$ $P="100 kPa"$
$V = ? ? ?$ $V= ???$
$n = {7 mol CH}_{4}$ $n="7 mol CH"_4"$
$R = {8.3144598 L kPa K}^{- 1} {mol}^{- 1}$ $R="8.3144598 L kPa K"^(−1) "mol"^(−1)"$
$T = 273.15 K$ $T="273.15 K"$

Equation
$P V = n R T$ $PV=nRT$

Solution
Rearrange the equation to isolate volume and solve.

$V = \frac{n R T}{P}$ $V=(nRT)/P$

$V=(7 cancel(mol) * 8.3144598"L" cancel"kPa" cancel"K"^(−1)""cancel"mol"^(−1) * 273.15cancel"K")/(100cancel"kPa")="159 L"="200 L CH"_4"$ (rounded to one significant figure)

Science

Math

Humanities

... and beyond

How would you find the volume of 7 moles of CH4 at standard temperature and pressure?

1 Answer

Explanation:

Related questions

Impact of this question