A gas occupies 1.00cm^3 at STP. What volume does it occupy at 710.0 mm Hg and 55.0°C

Final volume is 1.29cm³

Explanation:

Using combined gas law:

P₁V₁/T₁ = P₂V₂/T₂

Where P is pressure, V volume and T absolute temperature of 1, initial state and 2, final state of a gas.

We can solve the volume of the gas:

P₁ = 1atm at STP

V₁ = 1cm³

T₁ = 273.15K at STP

P₂ = 710mmHg * (1atm / 760mmHg) = 0.9342atm

V₂ = ?

T₂ = 55.0°C + 273.15K = 328.15K

Replacing:

1atm*1cm³/273.15K = 0.9342atm*V₂/328.15K

1.29cm³ = V₂

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explanation:

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.