What is the pressure of a 34.8-L gas sample containing 7.45 mol of gas at 19.9°C? (R = 0.0821 L • atm/(K • mol),1 atm = 760 torr) A)2.66 × 10² mmHg B)6.77× 10^-3 mmHg C)5.14 mmHg D)3.91 × 10³ mmHg E)1.48 × 10² mmHg

Question

Quizplus · Accepted Answer

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

T = 19.9°C + 273.15 = 293.05 K

Next, we can use the ideal gas law to calculate the pressure:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin.

Rearranging the equation to solve for P gives:

P = nRT/V

Plugging in the given values, we get:

P = (7.45 mol)(0.0821 L•atm/(K•mol))(293.05 K)/(34.8 L)
P = 3.91 × 10²³ atm ≈ 3.91 × 10³ torr ≈ 3.91 × 10¹³ mmHg

We can then round our answer to two significant figures, which gives:

P = 3.9 × 10¹³ mmHg

Therefore, the best answer choice is D: 3.91 × 10¹³ mmHg.

What Is the Pressure of a 34