Answer to Question #334170 in Chemistry for shimmy

Question

Solve: What will be the final volume of a 5.00 L He gas which contains 0.965 mole at 30°C and 1.00 atmosphere, if the amount of this gas is increased to 1.80 moles provided that the temperature and pressure remains unchanged?

Given: V₁ = 5.00L                                                       V₂ = ?

_T𝟏 = 0.965 mole                                            T_𝟐 = 1.80 moles

Answer 1

Given:

P₁ = P₂ = 1.00 atm = constant

T₁ = T₂ = 30°C = constant

n₁ = 0.965 mol

V₁ = 5.00 L

n₂ = 1.80 mol

V₂ = unknown

Formula: V₁ / n₁ = V₂ / n₂

Solution:

Since the temperature and pressure remain unchanged, Avogadro's law can be used.

Avogadro's law can be expressed as: V₁ / n₁ = V₂ / n₂

V₁n₂ = V₂n₁

To find the final volume, solve the equation for V₂:

V₂ = V₁n₂ / n₁

V₂ = (5.00 L × 1.80 mol) / (0.965 mol) = 9.3264 atm = 9.33 atm

V₂ = 9.33 atm

Answer: The final volume of He gas will be 9.33 atm