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.

You use the atomic number to find out how many protons and neutrons there are in the atom. you use the atomic mass to find out how many protons and electrons there are in the atom.