Question

If 63.1 g of NH3 occupies 35.1 L under a pressure of 93.1 in. Hg, what is the temperature of the gas, in °C?

Answer 1

PV=nRT, so since n and R are constant here, PV/T is constant.

1atm = 29.9 in Hg, and 1 mole occupies 22.4L at STP, so you want T such that
(93.1)(35.1)/(T+273.15) = (29.9)(63.1/17 * 22.4)/(273.15)

Answer 2

The following appears to me to be a much simpler way to solve the problem. Stick with PV = nRT

P = 93.1 inches x 1 atm/29.9 inches = 3.12 atm
V = 35.1 L
T= ?
n = 63.1g/17 = 3.72
R = 0.0821
3.12*35.1 = 3.72*0.0821*T
T = 359 K. Then 359- 273 = 86 C

Answer 3

As usual, DrBob222 cuts to the chase.

Luckily, my little calculation agrees with his!

Answer 4

Yes, the answers agree. I checked that FIRST THING because I know oobleck is always right.

Answer 5

[AI-generated answer — Explain Bot]

To find the temperature of the gas, you can use the ideal gas law equation:

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.

First, we need to convert the given pressure from inches of mercury (in. Hg) to atmospheres (atm). Since 1 atm = 29.92 in. Hg, we can convert 93.1 in. Hg to atm:

93.1 in. Hg * (1 atm / 29.92 in. Hg) = 3.11 atm (rounded to two decimal places)

Next, we need to calculate the number of moles (n) of NH3 using its mass and molar mass. The molar mass of NH3 is 17.03 g/mol (14.01 g/mol for nitrogen + 3 * 1.01 g/mol for hydrogen):

63.1 g NH3 * (1 mol NH3 / 17.03 g NH3) ≈ 3.70 mol NH3 (rounded to two decimal places)

Now we can rearrange the ideal gas law equation to solve for temperature (T):

T = PV / nR

Substituting the values we have:

T = (3.11 atm) * (35.1 L) / (3.70 mol) * (0.0821 L * atm / K * mol)

Simplifying:

T ≈ 286 K (rounded to the nearest whole number)

Finally, to convert the temperature to Celsius, you subtract 273.15 from the Kelvin value:

T in °C = 286 K - 273.15 ≈ 12.85 °C (rounded to two decimal places)

Therefore, the temperature of the gas is approximately 12.85 °C.