Question

A sample of helium gas occupies 13.1 L at 23 °C and 0.956 atm. What volume will it occupy at 40 °C and 1.20 atm? * 17.4 L 11.0 L 9.87 L 18.2 L 13.2 L

Answer 1

Explanation:

P

1

V

1

T

1

=

P

2

V

2

T

2

, which is the combined gas law? Temperature is specified to be on the

absolute scale

.

So,

V

2

=

P

1

×

V

1

×

T

2

T

1

×

P

2

=

0.956

⋅

a

t

m

×

14.7

⋅

L

×

313

⋅

K

300

⋅

K

×

1.20

⋅

a

t

m

Answer 2

Answer:

Answer will be 11.14 L ( or 11.0 L by rounding it off )

Explanation:

P₁ = 0.956atm

V₁ = 13.1 L

T₁ = 23℃= 296 K

P₂ = 1.2 atm

V₂ = ?

T₂ = 40℃

According to Gas Equation,

(P₁ × V₁) ÷ T₁ = (P₂ × V₂) ÷ T₂

⟹ ( V₁ × P₁ × T₂ ) ÷ ( T₁ × P₂ ) = V₂

⟹ ( 13.1 × 0.956 × 316 ) ÷ ( 296 × 1.20 ) = V₂

⟹ 11.14 = V₂

∴ V₂ = 11.14 L ( or 11.0 L )

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