If 0.357 g of CH₄ gas is introduced into an empty 1.75 L flask at 25 °C,what will be the pressure inside the flask? (R = 0.08206 L⋅atm/mol⋅K) A) 0.952 atm B) 0.261 atm C) 0.311 atm D) 0.419 atm E) 4.99 atm

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of the gas:

n = m/M = 0.357 g / 78.17 g/mol = 0.00456 mol

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

PV = nRT

P = nRT/V

P = (0.00456 mol)(0.08206 L·atm/mol·K)(298 K)/(1.75 L)

P = 0.311 atm

Therefore, the pressure inside the flask is 0.311 atm. The answer is C).

If 0357 G of CH4 Gas Is Introduced into an Empty

If 0357 G of CH₄ Gas Is Introduced into an Empty