Acompound of carbon and hydrogen contains 85.63% c and has a molar mass of 56.10 g/mol. what is its molecular formula? 

The empirical formula of the compound is calculated as follows:

Given that  

It contains 85.63% carbon,  and 100-85.63=  14.37 % hydrogen  

now assume that the amount of compound is100 g thus there is 85.63 g C and  14.37 g H

NOW  divide these percentages by the molar mass of the elements to get a number of moles for each substance.  

NUMBER OF MOLES = AMOUNT IN G / MOLAR MASS

Carbon: 85.63/12 = 7.1  

Hydrogen: 14.37/1 = 14.3  

Now arrange these in a ratio as follows:  

C:H

7.1/7.1 :14.3/7.1

1:2

divide through by the smallest number

Therefore, the empirical formula is CH2

Then calculate the molar mass of that molecule:  

(1x12) + (2x1) = 14

Here the molar mass of compound is  56.10 g/mol

Since, 14 goes into 56.10 g/mol  4 times thus the  molecular formula is : C4H8

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.