A gas sample at 40.0*C occupies a volume of 2.32 L. If the temperature is raised to 75*C, what will the volume be, assuming the pressure remains constant?

The final volume of the gas sample at the given condition is 2.58 L.

The given parameters:

The final volume of the gas is calculated by applying Charles law as shown below;

Thus, the final volume of the gas sample at the given condition is 2.58 L.

Learn more about Charles law here: link

2.58L

Explanation:

We must convert the temperature from °C to Kelvin temperature

T1 = 40°C = 40 + 273 = 313K

V1 = 2.32 L

T2 = 75°C = 75 + 273 = 348K

V2 = ?

V1 /T1 = V2 /T2

2.32 / 313 = V2 / 348

Cross multiply to express in linear form

313 x V2 = 2.32 x 348

Divide both side by the coefficient of V2 ie 313. We have

V2 = (2.32 x 348) /313

V2 = 2.58L

Therefore, if the temperature is raised to 75°C, the volume of the gas will be 2.58L

hi,

the answer is d, it has indefinite shape but definite volume.

hope this !

"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"