Zn + 2HCl ---> H2 + ZnCl2
n = 0.112
mw = 65.39
g = 7.35
From these values (they are for the zinc), you can see that only .112 mol of Zn reacted.
To find the number of moles of HCl, we use n = cV.
n = 1.2 x 0.5
= 0.6 x 2 mols
= 1.2 mol HCl.
From this we can see that zinc is the limiting reagent and that 0.112 mol of H2 gas was produced.
g = mw x n
g = 2.016 x 0.112
= 0.225792 grams.
Balanced equation first.
Zn + 2HNO3 >> Zn(NO3)2 + H2
( I forgot STP conversion, so I will use the trusty PV = nRT )
(1atm)(75.5l) = n(0.08206Latm/molK)(273.15K)
n (moles) = 3.37 moles H2
3.37 moles H2 (1mol Zn/1mol H2)(65.41g Zn/1mol Zn)
= 220.47 grams Zn needed.
Balanced equation.
2Al + 6HCl -> 2AlCl3 + 3H2
find moles hydrogen gas
2.70 grams Al (1 mole Al/26.98 grams)(3 moles H2/2 mole H2)
= 0.10007 moles H2
Now use PV = nRT
(1 atm)(volume H2) = (0.10007 moles H2)(0.08206 L*atm/mol*K)(298.15 K)
= 2.45 Liters of hydrogen gas
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2.50 g Zn * (1 mol Zn/65.39 g Zn) * (1 mol H2/ 1 mol Zn) * ( 22.4 L H2/1 mol H2) = 0.856 L of H2
The answer is 23L. There is 25.0 g of excess reagent that is left over in that problem.
23
14.9cm^3
Assuming that hydrogen, chlorine, and hydrogen chloride are all ideal gases and that the temperature and pressure are kept constant, the volume of gas depends only on the number of molecules of gas present. Also, at standard temperature and pressure, hydrogen and chlorine occur as diatomic molecules, and hydrogen chloride also occurs as diatomic molecules. The equation for the reaction is Cl2 + H2 -> 2 HCl. Therefore, the number of molecules of gas is the same before and after the reaction if both gases are present in the initial mixture that has a volume of 40 cm3. In that instance, the volume is the same before and after the reaction. However, the question seems to imply that hydrogen is supplied from an outside source. In that instance, there will be twice as many molecules after the reaction as before, so that the final volume will be 80 cm3.
The volume of hydrogen produced would stay the same because there is already plenty of water needed to react with 0.1 mol of Calcium.
The strength of a solution may be described as a percentage or volume, where 1% hydrogen peroxide releases 3.3 volumes of oxygen during decomposition.Thus, a 3% solution is equivalent to 10 volume and a 6% solution to 20 volume, etc. Answer taken from Wikipedia 19/01/2009
This means that for every volume of hydrogen peroxide used, 20 volumes of oxygen will be produced. For example, if 1 ml of hydrogen peroxide is used/decomposes, 20 ml of oxygen will be formed.
30% of weight by volume(w/v) hydrogen peroxide or 100 volume strength hydrogen peroxide is perhydrol.
The chemical reaction is:Ca + H2SO4 = CaSO4 + H2The volume of released hydrogen is 66,6 L.
The reaction is:Zn + HCl = ZnCl2 + H2The volume of hydrogen ia 1,7 L.
67.2
Assuming that hydrogen, chlorine, and hydrogen chloride are all ideal gases and that the temperature and pressure are kept constant, the volume of gas depends only on the number of molecules of gas present. Also, at standard temperature and pressure, hydrogen and chlorine occur as diatomic molecules, and hydrogen chloride also occurs as diatomic molecules. The equation for the reaction is Cl2 + H2 -> 2 HCl. Therefore, the number of molecules of gas is the same before and after the reaction if both gases are present in the initial mixture that has a volume of 40 cm3. In that instance, the volume is the same before and after the reaction. However, the question seems to imply that hydrogen is supplied from an outside source. In that instance, there will be twice as many molecules after the reaction as before, so that the final volume will be 80 cm3.
Hydrogen is produced when Al or Mg is allow to react with acids. Hydrogen is produced in the reactions of aluminum with sodium hydroxide but not with Mg (the reaction of Al with NaOH is used for the determination of aluminum in some alloys and mixtures, measuring the volume of hydrogen evolved.) with hot water Mg produces hydrogen but Al does not
Yes but might depend on the reaction, assuming you mean the production of hydrogen from a reaction of an acid and metal, the higher concentration of acid would mean there are more H+ ions in the solution therefore there would be a higher volume of gas produced.
Because the electrolysis of water reaction always produces twice as much hydrogen (by volume or by mole) as they do oxygen. H2O(l) -> H2(g) + 1/2 O2(g)
The molar volume of hydrogen is approx. 22,7 L at 100 kPa and 0C.
If the chemical reaction is:2 HCl + Mg = MgCl2 + 2 H23143 moles of HCl produce 3143 moles of hydrogenThis volume at 0 0C is70 447,202litres.
The volume is 50 %.
The volume of hydrogen produced would stay the same because there is already plenty of water needed to react with 0.1 mol of Calcium.
The reaction equation is: 2H2 + O2 = 2H2O So one need two volume part of hydrogen and one volume part of oxygen to form water.