A sample with a molar mass of 34.00 g/mol is found to consist of 5.9783% Hydrogen and 94.0217% oxygen. Find it’s molecular formula.

The formula is H202 (hydrogen peroxide, known as hydrogen peroxide)

Explanation:

100%34g

5, 9783%---X= (5, 9783%x 34g)/100% =2 g

1g---1 atom of H

2gx= 2g x 1 atom of H/1g = 2 atom of H

100%34g

94, 0217%---X= (94,0217%x 34g)/100% =32 g

16g---1 atom of 0

32gx= 32g x 1 atom of 0/16g = 2 atom of 0

what are the statements

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2