1. A sample of argon gas is at a pressure of 1.24 x 10^4 kPa and a temperature of 24°C in a rigid 25-L tank. How many moles of argon does this tank contain?

I ended up with .130 but its 130

Can someone tell me what I did wrong?
This whole chapter on gases is really confusing to me and it would help if someone explained it

Possibly the conversion of kPa? Which gas constant did you use?

As an estimate

1.24 x 10^ 4 kPa is approximately 124 atmospheres.

If 1 mole of a gas occupies 22.4 L at STP

Then the number of moles is very approximately

124 x 25/22.4 moles = 138 moles

PS - remember to include the leading zero when writing a decimal as the dot is very easy to miss.

Well, it sounds like you might have made an error in your calculations. Let's figure this out together!

To solve this problem, we can use the ideal gas law, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin. To do that, just add 273 to the temperature in Celsius. In this case, 24°C + 273 = 297K.

Now, let's plug the values into the formula and solve for n.

P = 1.24 x 10^4 kPa
V = 25 L
R = 8.314 J/(mol·K)
T = 297 K

(1.24 x 10^4 kPa) · (25 L) = n · (8.314 J/(mol·K)) · (297 K)

Simplifying this equation will give you:

n = (1.24 x 10^4 kPa) · (25 L) / (8.314 J/(mol·K)) · (297 K)

Now, let's crunch the numbers:

n ≈ 0.1298 mol

So, the number of moles of argon in the tank is approximately 0.1298 mol, which is really close to your initial answer of 0.130 mol. It seems like you were on the right track, so don't be too hard on yourself!

Remember, the ideal gas law can be a bit tricky, but with practice, you'll get the hang of it. And don't hesitate to ask for help if you're still feeling confused. Gases can be quite "pressure-sing," after all!

To determine the number of moles of argon gas in the tank, you can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in Pascals)
V = volume (in cubic meters)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)

To start, you need to convert the given pressure and temperature to units that can be used in the equation.

1. Convert the pressure from kPa to Pascals:
1.24 x 10^4 kPa = 1.24 x 10^4 × 1000 Pa = 1.24 x 10^7 Pa

2. Convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273
T = 24°C + 273 = 297 K

Now, let's plug in the values into the ideal gas law equation:

(1.24 x 10^7 Pa) * (25 L) = n * (8.314 J/(mol·K)) * (297 K)

Note: The volume should be converted from liters to cubic meters (since R is in SI units):

25 L = 25 * 0.001 m^3 = 0.025 m^3

(1.24 x 10^7 Pa) * (0.025 m^3) = n * (8.314 J/(mol·K)) * (297 K)

To solve for n, rearrange the equation:

n = (1.24 x 10^7 Pa * 0.025 m^3) / (8.314 J/(mol·K) * 297 K)

Now, calculate the value using a calculator:

n ≈ 0.1305 mol

Therefore, the tank contains approximately 0.1305 moles of argon gas.

It seems that the value you obtained is correct (0.130), so there might have been a mistake in the conversion or calculation. Double-check each step to ensure all units and values are correct.

To find the number of moles of argon gas in the tank, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure in atmospheres (convert kPa to atm)
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin (convert °C to Kelvin)

Let's go through the calculations step by step:

1. Convert the pressure from kPa to atm:
1.24 x 10^4 kPa * (1 atm / 101.3 kPa) = 122.3666 atm (approximately)

2. Convert the temperature from °C to Kelvin:
24°C + 273.15 = 297.15 K

3. Plug in the values into the ideal gas law equation:
(122.3666 atm) * (25 L) = n * (0.0821 L·atm/(mol·K)) * (297.15 K)

4. Solve for n, the number of moles:
n = (122.3666 atm * 25 L) / (0.0821 L·atm/(mol·K) * 297.15 K)
n ≈ 131 moles

Therefore, the tank contains approximately 131 moles of argon gas.

If you obtained a different result, you might have made a rounding error during the calculations or used incorrect conversion factors. Make sure to double-check each step and use the correct units for pressure, volume, and temperature.