How hot would a 2.3 l balloon have to get to expand to a volume of 3.0 l? assume the initial temperature of the balloon is 24 °c, and that the pressure inside the balloon remains constant. a. 3 k b. 42 k c. 128 k d. 390 k

This question calls for Charles' Law (one of the gas laws) because it deals with volume and temperature of a gas. Charles' Law is as follows:
V₁/T₁ = V₂/T₂
Just plug in what you know! The initial volume and temperature (V₁ and T₁) are 2.3L and 24⁰C. The final volume (V₂) is 3.0L. Solve for T₂ algebraically:
2.3/24 = 3.0/T₂ *cross multiply here
2.3T₂ = 72
T₂ = 31.3⁰C
Now, convert to Kelvin by adding 273 to the temperature.
31.3 + 273 = 304.3K
The answer must be D because that is the only option where the balloon would reach at least 3.0L.

Ethene molecular fórmula= c2h4molecular weight = 29.046g/molhope it : )

Ch4 is nonpolar and insoluble in water. since all of the hydrogen atoms are evenly spread around the carbon atom even through the c h bond is polar all the poles cancel each other out.