Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2(s) + 2H2O(l) → Sr(OH)2(s) + 2H2(g)

You wish to calculate the mass of hydrogen gas that can be prepared from 4.67 g of SrH2 and 3.89 g of H2O.

(a) How many moles of H2 can be produced from the given mass of SrH2?
moles
(b) How many moles of H2 can be produced from the given mass of H2O?
moles
(c) Which is the limiting reactant?

SrH2

H2O
(d) How many grams of H2 can be produced?

Lab reagent, hypothesis test.a reference solution used as a lab reagent is purported to have a concentration of 5 mg/dl. six samples are taken from this solution and the following concentrations are recorded: (5.32, 4.88, 5.10, 4.73, 5.15, 4.75) mg/dl.these six measurements are assumed to be an srs of all possible measurements from solution.they are also assumed to have a standard deviation of 0.2, a normal distributin, and a mean concentration equal to the true concentration of the solution.carry out a significance test to determine whether these six measurements provide reliable evidence that the true concentration of the solution is actually not 5 mg/dl.

How many moles are contained in 5.6 l of h2 at stp

8. what happens to matter during a chemical reaction