a balloon is filled with .50 moles out of gas at room temp and normal room pressure, the balloon volume would be 11.2L. if you heat the balloon keeping the room pressure and amount of gas unchanging, what would be the effect on the volume of the balloon?

The ideal gas law states that for n moles of gas, the following relation applies:

PV=nRT
where
P=pressure
V=volume
R=constant
T=temperature in °K

In the present case,
P and n (and R) remain constant, from which we can conclude that the volume varies directly proportional to the temperature of the gaz (in °K).

Note: temp. in °K = temperature in °C+273.15

To understand the effect of heating on the volume of the balloon, we need to recall the ideal gas law. The ideal gas law equation is given by:

PV = nRT,

where P represents pressure, V represents volume, n represents the number of moles of gas, R is the ideal gas constant, and T represents the temperature in Kelvin.

In this case, you have mentioned that the number of moles of gas (n) and the pressure (P) are kept constant while heating the balloon. Therefore, the equation becomes:

V1/T1 = V2/T2,

where V1 is the initial volume of the balloon at room temperature, T1 is the initial temperature, V2 is the final volume of the balloon after heating, and T2 is the final temperature.

We are given that the initial volume (V1) is 11.2 L. Since the amount of gas and pressure remain constant, we can rewrite the equation as:

V1/T1 = V2/T2,

Substituting the values, we get:

11.2 L / T1 = V2 / T2.

Now, since we are considering the change in volume, we can rearrange the equation as:

V2 = (T2 / T1) * 11.2 L.

From the equation, we can conclude that as the temperature (T2) increases, the volume of the balloon (V2) will also increase, as long as the initial volume, pressure, and the amount of gas are held constant.

In summary, heating the balloon while keeping the amount of gas and pressure constant will result in an increase in the volume of the balloon. The relationship between the volume and temperature is directly proportional according to the ideal gas law.