0,75 grams hydrogen
The balanced equation for the reaction between Iodine and Hydrogen is: H2 + I2 --> 2HI The ratio of I2 to HI is 1:2 Therefore 1 mole of Iodine can form a maximum of 2 moles of Hydrogen Iodide
6H2 + 6O2 ---> 6H2O + 3O2 This reaction leave excess unreacted oxygen behind.
To find the mass of hydrogen gas produced, start by determining the moles of magnesium reacting by dividing the mass of magnesium by its molar mass. Then, use the balanced chemical equation to find the moles of hydrogen gas produced, as it is a 1:1 ratio with magnesium. Lastly, convert the moles of hydrogen gas to grams to find the mass.
The reaction between magnesium and hydrochloric acid produces hydrogen gas according to the equation: Mg + 2HCl -> MgCl2 + H2. For every 1 mole of magnesium reacted, 1 mole of hydrogen gas is produced. Using the molar mass of hydrogen (1 g/mol), the mass of hydrogen produced would be 1 gram when 1 mole of magnesium is reacted.
The reaction between aluminum metal and hydrochloric acid produces hydrogen gas and aluminum chloride. To find the volume of hydrogen gas produced, you would need to know the molarity of the hydrochloric acid and the temperature and pressure of the reaction. Once you have that information, you can use the ideal gas law to calculate the volume of hydrogen gas produced.
The reaction is:WO3 + 3 H2 = W + 3 H2OThree moles of hydrogen for one mole of wolfram.
When acids in water hydrogen positive ion is produced in excess. It is this hydrogen positive ion that gives acidity of a solution.
The excess of neutrons produced.
Since 1 mole of O2 reacts with 2 moles of hydrogen to produce 2 moles of water, 250 moles of O2 will produce 500 moles of water. Assuming ideal gas behavior and STP conditions, 1 mole of gas occupies 22.4 L, so 500 moles of water will occupy 11,200 liters.
Hydrotreating reaction is an exothermic reaction. The total reaction provides excess reaction heat; more is produced by the exothermic hydrogenation reactions than are required to support the endothermic cracking reactions.High Olefin conc. leads to high temp. rise due to hydrogenation reaction.This excess heat increases the reactor temperature and accelerates the reaction rate. Temperature rise can be controlled by injecting cold hydrogen or cold recycled quench into the reactors to absorb excess reaction heat.
No, both magnesium and zinc produce the same amount of hydrogen when the same amounts react with excess of strong acid (on molecular base), though the second reaction is slower. The reaction equations can tell you more about why this is.Mg + 2H+ --> Mg2+ + H2Zn + 2H+ --> Zn2+ + H2
To find the mass of hydrogen gas produced, start by determining the moles of magnesium reacting by dividing the mass of magnesium by its molar mass. Then, use the balanced chemical equation to find the moles of hydrogen gas produced, as it is a 1:1 ratio with magnesium. Lastly, convert the moles of hydrogen gas to grams to find the mass.
6 moles
6H2 + 6O2 ---> 6H2O + 3O2 This reaction leave excess unreacted oxygen behind.
Balanced equation first. N2 + 3H2 >> 2NH3 (hydrogen is limiting and drives the reaction ) 3.41 grams H2 (1mol/2.016g )(2mol NH3/3mol H2 )(17.034g NH3/1mol NH3 ) = 19.2 grams of ammonia produced ( this is called the Born-Haber process )
N2 + 3H2 --> 2NH3 You have been told, indirectly, that nitrogen limits and will drive the reaction. 3 moles N2 (2 moles NH3/1 mole N2) = 6 moles ammonia gas produced ========================
To find the moles of HCl, first convert 250.0 mL to liters (0.250 L). Then, use the molarity (3.0 M) to calculate moles of HCl: 0.250 L x 3.0 mol/L = 0.75 moles of HCl. Since Mg is in excess, all HCl will react. The balanced equation is 2HCl + Mg -> MgCl2 + H2, so 0.75 moles of HCl will produce 0.75 moles of H2 gas.