Aballoon initially has a volume of 45 l at sea level, where temperature is 25∘c and the pressure is 1.0 atm. it rises to an elevation of 2.0 km, where the temperature is 5.0∘c and the pressure is 0.78 atm. what is the balloon's volume at this height?

The answer to your question is Volume = 11.54 liters

Step-by-step explanation:

Data

Initial volume = V1 = 45 l

Temperature 1 = T1 = 25°C

Pressure 1 = P1 = 1 atm

Temperature 2 = T2 = 5 °C

Pressure 2 = P2 = 0.78 atm

Volume 2 = V2 = ?

Process

Use the combined law of gases to solve it

Solve for V2

Substitution

Simplification

Result

                  V2 = 11.54 liters

part a

x     y

0     8

1     7.5

2     7

3     6.5

4     6

5     5.5  

for every hour i deducted .5 inches from the length of the candle

part b

it is a function because for every x value there is only one y value

part   c

for every x value there is only one y value

x       y

0       8

1       7.6

2       7.2

3       6.8

step-by-step explanation:

step-by-step explanation:

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