Question 5
3 p
a gas cylinder with a volume of 15,0 liters contains 1.75 moles of nitrogen gas at 17.50c. what is the pressure inside the cylinder?
show all of your work for the following problems, including unit conversions, for full credit. pay attention to the significant digits and the units.

The pressure inside the cylinder will be 2.78 atm. The pressure can be calculated using the Ideal Gas Equation which relates the pressure, volume, temperature, and amount of gas to each other.  

Further Explanation

The Ideal Gas Equation is:  

where:

P - pressure (in atm)

V - volume (in L)

n - amount of gas (in moles)

R - universal gas constant

T - temperature (in K)

In the problem, we are given the values:

P = ?

V = 15.0 L (3 significant figures)

n = 1.75 moles N2 ( 3 significant figures)

T = 17.50 degrees Celsius (4 significant figures)

We need to convert the temperature to Kelvin before we can use the Ideal Gas Equation. The formula to convert from degree Celsius to Kelvin is:

Therefore, for this problem,

Solving for P using the Ideal Gas Equation:

The least number of significant figures is 3, therefore, the final answer must have only 3 significant figures (P = 2.78 atm).

Learn More

1. Learn more about Boyle's Law  

2. Learn more about Charles' Law

3. Learn more about Avogadro's Law

Keywords: Ideal Gas Law, Gas 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"