Answer:
9.6 moles O2
Explanation:
I'll assume it is 345 grams, not gratis, of water. Hydrogen's molar mass is 1.01, not 101.
The molar mass of water is 18.0 grams/mole.
Therefore: (345g)/(18.0 g/mole) = 19.17 or 19.2 moles water (3 sig figs).
The balanced equation states that: 2H20 ⇒ 2H2 +02
It promises that we'll get 1 mole of oxygen for every 2 moles of H2O, a molar ratio of 1/2.
get (1 mole O2/2 moles H2O)*(19.2 moles H2O) or 9.6 moles O2
That's cool man, you should study more... wheres the question though?
Answer:
Explanation: so a combustion occurs when we react a substance with oxygen .you commonly call this "burning'' .therefore combustion will always include oxygen in the equation and the product will include carbon dioxide and give off water vapours
Therefore the general equation for a complete combustion reaction would be
Fuel + O2 ------ CO2 + H2O
Answer:
The correct option is: A. activity; concentration
Explanation:
A reaction rate essay is a laboratory method to determine the activity of an enzyme. It is necessary for determining the enzyme kinetics and inhibition.
Whereas, a colorimetric analysis is a method to determine the concentration of a chemical compound in a solution. Therefore, a colorimetric endpoint assay measures the concentration.
Therefore, Enzyme activity is measured by a reaction rate assay and the concentration is measured by a colorimetric endpoint assay.
V( H₂SO₄) = 25.0 mL in liters = 25.0 / 1000 = 0.025 L
M(H₂SO₄) = ?
V(NaOH) = 50.0 mL = 50.0 / 1000 = 0.05 L
M(NaOH) = 0.150 M
number of moles NaOH :
n = M x V
n = 0.150 x <span> 0.05
</span>
n = 0.0075 moles of NaOH
H₂SO₄(aq) + 2 NaOH(aq) = Na₂SO₄(aq) + 2 H₂O(l)
1 mole H₂SO₄ ---------- 2 mole NaOH
? mole H₂SO₄ ---------- 0.0075 moles NaOH
moles = 0.0075 * 1 / 2
= 0.00375 moles of H₂SO₄
M(H₂SO₄) = n / V
M = 0.00375 / <span> 0.025
</span>= 0<span>.15 M
</span>
hope this helps!
