A sample of gas at a pressure of 5.1 atm and a temperature of 45 degrees celsius is heated. it’s pressure goes to 7.8 atm what is it’s new temperature in celsius

213.4°C.

Explanation:

Data obtained from the question:

Initial pressure (P1) = 5.1atm

Initial temperature (T1) = 45°C = 45°C + 273 = 318K

Final pressure (P2) = 7.8atm

Final temperature (T2) =..?

The new temperature can be obtained as follow:

P1/T1 = P2 /T2

5.1/318 = 7.8/T2

Cross multiply

5.1 x T2 = 318 x 7. 8

Divide both side by 5.1

T2 = 318 x 7. 8 /5.1

T2 = 486.4K

Finally, we shall convert 486.4K to celsius temperature. This can be done as follow:

T(°C) = T(K) – 273

T(K) = 486.4K

T(°C) = 486.4 – 273

T(°C) = 213.4°C.

Therefore, the new temperature is 213.4°C

precipitation

explanation:

when it goes from cloud to rain/back to earth in the form of rain

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%