A tank contains 1500 L of argon gas. The pressure is 11690 kPa and the temperature is 35ºC. How many moles of argon are in the tank? Show your work

Question

asked Oct 7, 2024 85.1k views

2 Answers

Patrick Lorio · Answer 1 · 2024-10-10T01:28:07+0000

Answer: 6,847.7 moles of Argon Gas

Step-by-step explanation:

For this question, you need to use the Ideal Gas Equation (PV = nRT).

P is pressure (commonly in kPa or atm)
V is volume occupied by the gas (in L)
n is the number of moles, aka what we're trying to find here.
R is the Ideal gas constant (8.314 (kPa*L)/(mol*K), or 0.0821 (atm*L)/(mol*K)
T is the temperature (in Kelvins (K). In order to convert from Celsius to Kelvin, just add 273.)

We can rearrange this equation to calculate the number of moles:

n = PV/RT

Then, we can plug in the values (Caution: we have to use 8.314 for our Ideal gas constant since P is in kPa for this question)

...and we have our answer! 6,847.7 moles of Argon Gas.

Also, make sure to adjust to significant figures!

Schnoedel · Answer 2 · 2024-10-10T19:39:45+0000

Answer:

6843.99 mol (2 d.p.)

Step-by-step explanation:

To calculate the number of moles of argon in the tank, we can use the Ideal Gas Law.

$\boxed{PV=nRT}$

where:

First convert the given temperature from Celsius to kelvin by adding 273.15:

$\implies \sf T=35+273.15=308.15\;K$

Therefore, the values to substitute into the equation are:

Rearrange the formula to isolate n:

$\implies n=(PV)/(RT)$

Substitute the values into the formula and solve for n:

$\implies n=(11690 \cdot 1500)/(8.3144626... \cdot 308.15)$

$\implies n=(17535000)/(2562.10165...)$

$\implies n=6843.99073...$

$\implies n=6843.99\; \sf mol\;(2\;d.p.)$

Therefore, there are 6843.99 moles of argon in the tank (to two decimal places).