A gas exerts a pressure of 350.0 torr at 20.0 Celsius. What would be the new pressure in atmospheres if the temperature is raised to 40.0 Celsius

0.49 atm

Explanation:

Step 1:

Data obtained from the question. This includes:

Initial pressure = 350.0 torr

Initial temperature (T1) = 20°C

Final temperature (T2) = 40°C

Final pressure (P2) =?

Step 2:

Conversion to appropriate unit.

It is so vital to convert the units of the variable given to the appropriate unit in order to obtain the desired answer in the right unit. This is illustrated below:

For pressure:

760 torr = 1 atm

Therefore, 350 torr = 350/760 = 0.46 atm

For temperature:

Temperature (Kelvin) = temperature (celsius) + 273

T1 = 20°C = 20°C + 273 = 293K

T2 = 40°C = 40°C + 273 = 313K

Step 3:

Determination of the new pressure.

The new pressure can be obtained by applying the following equation:

P1/T1 = P2/T2

P = 0.46 atm

T1 = 293K

T2 = 313K

P2 =?

P1/T1 = P2/T2

0.46 / 293 = P2 / 313

Cross multiply to express in linear form

293 x P2 = 0.46 x 313

Divide both side by 293

P2 = (0.46 x 313) /293

P2 = 0.49 atm

Therefore, the new pressure is 0.49 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"