If the temperature of the helium balloon were increased from 30°C to 35°C and the volume of the balloon only expanded from 0.47L to 1.55L, how much pressure would be inside the balloon?

Explanation:

To solve this problem, we can use the Combined Gas Laws:

Data:

p₁ = p₁; V₁ = 0.47 L; n₁ = n₁;  T₁ = 30 °C

p₂ = ?;  V₂ = 1.55 L; n₂ = n₁; T₂ = 35 °C

Calculations:

(a) Convert the temperatures to kelvins

T₁ = (30 + 273.15)K = 303.15 K

T₂ = (35 + 273.15)K = 308.15 K

(b) Calculate the new pressure

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

answerto predict;