what mass of hydrogen peroxide must decompose to produce .7g of water?
96357
First figure out the chemical reaction,\n\nHydrogen PerOxide deomposes into water and Oxygen gas,\n2H2O2 --> 2H2O + O2\n\nYou now know that there is a 1:1 ratio for each mole of Hdrogen peroxide decomposing to form water.\nFor first figure out how many moles of water .7 grams if from the molar mass of water (18.02 g/mol) and then you know how many moles of H2O2.  The after you know the moles of H2O2 needed, convert to grams using the molar mass of Hydrogen PerOxide (34.02 g/mol).
598825
Peroxide is H2O2. If it were in a clear bottle, that second oxygen would evaporate and it would become H20...water.
865537
When silane burns, SiO2 is formed (and water). You can now draw up the balanced equation.\n\nManganese(IV) oxide catalyses the decomposition of hydrogen peroxide:\n\n2H2O2 ----> 2H2O + O2
212429
dots..\nits jux 2 hydrogen and 1 oxygen for every mole of h2o
1125360
H2O2 can exist in many forms at pH = 7, \n\nH3O2+, H3O3- are among the possibilities.
521993
Yes, hydrogen peroxide decomposes spontaneously into water and oxygen.  The decomposition is enhanced by exposure to heat, light, and contaminants.  So, over time, that bottle of 2% peroxide in your medicine cabinet will become nothing more than water (not that water is a bad thing).
215604
C6H12O6(s) ---H2SO4--> 6C(s) + 6H2O(in H2SO4 solu.) + Heat
878226
The method is very simple.  I can do the first and you can try the others.\n\n1.  First write the reaction and balance it.\n\n2HgO ---> 2Hg + O2.\n\n2. Convert grams to moles of whatever mass you have.  In this case you have O2 as 96 grams.  You convert to moles by dividing the mass by the molecular weight.  In this case, for O2 will be 32 g/mol\n\n96 grams / 32 g/mol = 3 mol.\n\n3. Now you look back to the equation.  In the equation for producing 1 mol O2 you need 2 moles of HgO.  If now have 3 moles O2, then you will need 2 x 3 moles of HgO, 6 moles.\n\n4. Now you need to convert the moles of HgO to grams.  To do this calculate the molecular weight of HgO.  It is 216.6 g/mol\n\n6 moles * 216.6 g/mol = 1299.6 g of HgO.
479787
In 100g of solution that is 5% by mass NaCl, there are 95 g H2O and 5g Nacl.\nYou want 250g of solution...set up a simple ratio:\n95g H2O/100g Soln = ?g H2O/250g Soln\n? = 237.5g H2O
247135
The formula for water is H2O i.e. there are 2 atoms of hydrogen and one atom of oxygen. Its molecular weight is 18 g/mol .
960502
Since the oxygen is collected over water, you must subtract out the water vapor pressure to determine the pressure due to just the oxygen.\n\n722.2 mmHg - 21.1 mmHg = 701.1 mmHg = 0.922 atm due to O2\n\n0.276g KClO3 = 0.00175 moles KClO3 (molar mass = 158 g/mol)\nSince KClO3 decomposes to form O2 in a 2:3 ratio, the number of moles of O2 produced = 0.00262 moles O2\n\nPV=nRT\n(0.922 atm) V  = 0.00262 mol (0.08206)(296.2K)\n\nSolving for the volume due to the O2,  V = 691 mL
929435
a drop of water weights  about  0.05 g \n\nThe molecular weight of water is 18 (H2 o = 2*1+16)\n\nso the number of moles of water in a drop is  0.05/18 =1.67 10^21 molecules
804845
yes u r correct , u need vapour pressure of H2O. From vapour pressure calculate vapour density of H2O\n  Now, u can easily calculate molecular mass of the unknown as it  is twice the vapour density
787311
A. H2O. Molecular water is 2H2O
736571
there are .833 moles. divide the mass by 18 (2 hydrogens + 1 oxygen) oxygen= 16g/mole Hydrogen = 1 g/mole
545577
H2(g)+ O3(g)=> H2O(L) + O2(g)\n\nBecause H2O is the prime factor of 02G if only 2H2 equals 2H20. If you take the "Smithy" equation into consideration and change the X into L factor, you will find that D is the correct answer!
969093
H2 = 2g/mol   2.05g = 1.025mol\nCO = 28g/mol    15.85g = .57mol\n\n2H2 + CO --> CH3OH\n\nmust be reduced to \nH2 + (1/2)CO --> (1/2)CH3OH\n\n1.025mol + (1/2).57mol --> the quantity of the limiting reactant which is .285mol CH3OH which at 32g/mol = 9.12g