Question

How many moles of Neon gas are there if 25.0 Liters of the gas are at 278K and pressure of 89.9 KPa (R= 8.314)

a
6.50 mol
b
0.97 mol
c
5.60 mol
d
0.85 mol

Answer 1

Answer:

(b) 0.97 mol

Step-by-step explanation:

We can use the Ideal Gas Law to solve this problem, which states that 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 given temperature of 278K to Kelvin. We have:

T = 278K

Next, we can plug in the values of the given pressure, volume, gas constant, and temperature into the Ideal Gas Law and solve for n:

PV = nRT

n = (PV) / (RT)

n = (89.9 kPa) x (25.0 L) / [(8.314 J/mol·K) x (278 K)]

n = 0.965 mol

Therefore, the answer is (b) 0.97 mol (rounded to two significant figures).