hydrogen and oxygen gas combine explosively to produce water. write a blanced equation for this process.
if 10 mol of hydrogen reacted with oxygen, what volume of liquid water could be produced?
balance the equation.
doesn't the balanced equation indicate 5 moles of water? how many grams is that? the density of water is 1gram/cc, so what volume is that?
for the answer
The balanced equation for the reaction between hydrogen and oxygen gas to produce water is:
2H₂ + O₂ → 2H₂O
To determine the volume of liquid water that could be produced when 10 mol of hydrogen reacts with oxygen, we need to use the concept of stoichiometry.
First, we need to find the stoichiometric ratio between hydrogen and water in the balanced equation, which is 2:2, meaning that 2 moles of hydrogen react to produce 2 moles of water.
Since we know that 10 moles of hydrogen are provided, we can set up a simple proportion to calculate the moles of water produced:
2 moles of hydrogen / 2 moles of water = 10 moles of hydrogen / x moles of water
Cross-multiplying, we get:
2x = 2 * 10
2x = 20
x = 20 / 2
x = 10
Therefore, 10 moles of water can be produced when 10 moles of hydrogen react. Keep in mind that this answer is in moles, not volume.
To determine the volume of water produced, we need to consider the ideal gas law, which states that:
PV = nRT
Where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. Since the reaction results in liquid water, we can generally assume that the volume of water is the same as the volume of the gases involved.
However, to get an accurate answer, we would need to know the temperature and pressure conditions under which the reaction is taking place.