Question

Suppose that 5.14 x 10-3 mol of hydrogen gas occupies a 1,171 mL container at 60°C. What is the pressure (in torr)? (Do not type the units.)

Answer 1

Answer:

91.2

Explanation:

Given that:

Temperature = 60 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T₁ = (60 + 273.15) K = 333.15 K  

n = 5.14 × 10⁻³ mol

V = 1,171 mL = 1.171 L ( 1 mL = 0.001 L)

Using ideal gas equation as:

$PV=nRT$

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 62.364 L Torr/ K mol  

Applying the equation as:

P × 1.171 L = 5.14 × 10⁻³ mol × 62.364 L Torr/ K mol  × 333.15 K  

⇒P = 91.2 torr