Consider a gas at 1.00 atm in a 5.00-L container at 20.0 °C. What pressure does the gas exert when transferred to a volume of 2.00 L at 43 °C?

The pressure is 2.696 atm

Explanation:

Boyle's law relates pressure and volume inversely proportionally and is expressed mathematically as:

P * V = k

Charles's law consists of the relationship between the volume and temperature of a certain amount of ideal gas, which is maintained at a constant pressure, by means of a proportionality constant that is applied directly and is expressed mathematically as follows:

Gay-Lussac's law indicates that the gas pressure is directly proportional to its temperature and is expressed mathematically as:

Combined law equation is the combination of three gas laws called Boyle's, Charlie's and Gay-Lusac's law:

When you want to study two different states, an initial and a final one of a gas, you have the expression:

In this case, you know:

Replacing:

Solving:

P2= 2.696 atm

The pressure is 2.696 atm

"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"

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be