An ideal gas has a pressure of 2.5 atm,a volume of 1.0 L at a temperature of 30°C.How many molecules are there in this gas? (R = 8.31 J/mol ∙ K,1.00 atm = 101 kPa,N_A = 6.022 × 10²³) A)6.1 × 10²³ B)6.0 × 10²² C)2.4 × 10²² D)2.3 × 10²³

Question

Quizplus · Accepted Answer

First, we need to convert the temperature from Celsius to Kelvin:

T (K) = 30°C + 273.15 = 303.15 K

Next, we can use the ideal gas law to calculate the number of moles of gas:

PV = nRT

where P = 2.5 atm, V = 1.0 L, R = 8.31 J/mol∙K, and T = 303.15 K.

Solving for n, we get:

n = PV/RT

n = (2.5 atm)(1.0 L)/(8.31 J/mol∙K)(303.15 K)

n = 0.000998 mol

Finally, we can use Avogadro's number to convert from moles to molecules:

number of molecules = (0.000998 mol)(6.022 × 10²³ molecules/mol)

number of molecules ≈ 6.0 × 10²² molecules

Therefore, the answer is B.

An Ideal Gas Has a Pressure of 2