10cm3 of hydrogen are burned in oxygen to form water.

What volume of oxygen is need to burn hydrogen completely?

To determine the volume of oxygen needed to burn hydrogen completely, we need to consider the balanced chemical equation for the combustion reaction of hydrogen and oxygen:

2H₂ + O₂ → 2H₂O

From the equation, we can see that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water. Since the balanced equation represents a ratio of moles, we need to convert the given volume of hydrogen (10 cm³) into moles before determining the volume of oxygen needed.

To convert volume to moles, we need to use the ideal gas law equation:

PV = nRT,

where P represents the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

Given:
Volume of hydrogen = 10 cm³

To convert cm³ to liters (L) and moles, we need to know the temperature and pressure. Let's assume standard temperature and pressure (STP):

Standard Temperature (T) = 273.15 K
Standard Pressure (P) = 1 atm

Using the ideal gas law at STP:

PV = nRT

Using the values:
P = 1 atm
V = 10 cm³
T = 273.15 K
R = 0.0821 L·atm/(mol·K)

We can solve for the number of moles:

n = (PV) / (RT)

n = (1 atm * 10 cm³) / (0.0821 L·atm/(mol·K) * 273.15 K)

Calculating this, we find:
n ≈ 0.004 mol

Now, since the balanced equation tells us that 2 moles of hydrogen react with 1 mole of oxygen, we can conclude that 0.004 moles of hydrogen require 0.002 moles of oxygen.

Finally, to convert moles to volume, we can use the same ideal gas law equation:

PV = nRT

Assuming the same temperature and pressure, let's assume the volume of oxygen is represented by V₂:

P₂ * V₂ = (0.002 mol) * (0.0821 L·atm/(mol·K)) * (273.15 K)

Solving for V₂:

V₂ = (0.002 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / P₂

Since the pressure is not provided, we cannot directly calculate the volume of oxygen needed without knowing the pressure. Please provide the pressure to proceed with the calculation.