How many grams of water are required to produce 5.50 l of hydrogen gas at 25.0°c and 755 mm hg pressure according to the chemical equation shown below?

4.014 g of water

Explanation:

An internet search for your question tells me that the chemical equation is:

So first we use PV=nRT to calculate the moles of hydrogen gas produced:

0.993 atm * 5.50 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 298.16 K

Now we convert mol H₂ to mol H₂O and finally to grams of water:

0.223 mol H₂ * = 4.014 g H₂O

plasma is the state of matter where the substance is ionized and has no definite shape or volume. the fact of being ionized makes the substance a good electrical conductor.

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