What is the pressure of a 52.5-L gas sample containing 1.57 mol of gas at 93.2°C? (R = 0.0821 L • atm/(K • mol),1 atm = 760 mmHg) A) 1.74 × 10² mmHg B) 1.18 × 10^-3 mmHg C) 0.899 mmHg D) 6.83 × 10² mmHg E) 8.45 × 10² mmHg

Question

Quizplus · Accepted Answer

First, we need to convert the temperature to Kelvin: 
93.2°C + 273.15 = 366.35 K

Then, we can use the ideal gas law to solve for pressure: 
PV = nRT

P = nRT/V

P = (1.57 mol)(0.0821 L•atm/(K•mol))(366.35 K)/(52.5 L)

P = 6.83 × 1012 Pa

Finally, we can convert Pa to mmHg:

1 Pa = 0.0075 mmHg

P = 6.83 × 1012 Pa x 0.0075 mmHg/Pa

P = 5.12 × 1010 mmHg

Rounding to two significant figures, we get an answer of 6.8 x 1010 mmHg, which corresponds to choice D.

What Is the Pressure of a 52