Consider a balloon that has a volume v. it contains n moles of gas, it has an internal pressure of p, and its temperature is t. if the balloon is heated to a temperature of 15.5t while it is placed under a high pressure of 15.5p, how does the volume of the balloon change? it doubles. it stays the same. it increases greatly. it decreases slightly.

It stays the same.

Explanation:

We should use the law of ideal gas to solve this problem: PV = nRTWhere, P is the pressure (atm), V is the volume (L), n is the number of moles, R is the general gas constant (0.082 L.atm/mol.K), and T is the temperature (K).For the same gas and in this problem; n and R are constants.The variables are P,V and T.For the two different cases (1&2): P₁V₁/T₁ = P₂V₂/T₂P₁ = P, V₁ = V and T₁ = T.P₂ = 15.5 P, V₂ = ??? and T = 15.5 T.To get the volume in the second case (V₂):V₂ = P₁V₁T₂/P₂T₁ = (P x V x 15,5 T) / (15.5 P x T) = V.So, the volume will stay the same.

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