2H20(l) = 2H2 (g) +O2 (g)
For the above, if 1.50 mg of water is decomposed, what mass of hydrogen is procduced? (1 Mg=10^6g=1 metric ton)?
What is the answer and what is the best way to solve this?
I am confused because you have used mg and Mg interchangeably. Here is the general procedure.
1. You have the balanced equation.
2. Convert grams water to moles. mols = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles H2O to moles H2.
4. Now convert moles H2 to grams. g = moles x molar mass.
I see your post piggy backed onto Jill's question. Repost here if you still have trouble.
Thanks for the info.
I came up with 0.1678475161 and rounded it to .17 mg H2. Am I on the right track and did I include the correct amount sig figs?
To solve this problem, we need to use the given balanced chemical equation and convert the given mass of water to the mass of hydrogen.
First, let's analyze the balanced chemical equation:
2H2O(l) → 2H2(g) + O2(g)
From the equation, we can see that 2 moles of water will produce 2 moles of hydrogen gas, so the stoichiometric ratio between water and hydrogen gas is 1:1.
Now, let's convert the given mass of water to moles. We are given that the mass of water is 1.50 mg.
1. Convert mg to grams:
1.50 mg x (1 g / 1000 mg) = 0.0015 g
2. Convert grams of water to moles of water using the molar mass of water:
0.0015 g H2O x (1 mol H2O / 18.015 g H2O) = 8.32 x 10^-5 mol H2O
Since the stoichiometric ratio between water and hydrogen gas is 1:1, the moles of hydrogen gas produced will be equal to the moles of water decomposed.
3. Convert moles of hydrogen gas to grams of hydrogen gas using the molar mass of hydrogen:
8.32 x 10^-5 mol H2 x (2.016 g H2 / 1 mol H2) = 0.000168 g H2
Finally, it is given that 1 Mg = 10^6 g. So, to convert grams to metric tons, we divide the result by 10^6.
0.000168 g H2 x (1 metric ton / 10^6 g) = 1.68 x 10^-10 metric ton H2
Therefore, the mass of hydrogen gas produced is 1.68 x 10^-10 metric ton.