Consider the chemical reaction
C + H2O -----> CO + H2
How many liters of hydrogen gas are formed From the complete reaction of 1.07 mol of C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and the temperature of 315K
So I'm looking for volume and I have a pressure and a temp now I'm lost please help
To determine the volume of hydrogen gas formed, we can use the ideal gas law:
PV = nRT
Where:
P = pressure (1.0 atm)
V = volume of gas (unknown)
n = number of moles of gas (unknown)
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (315 K)
First, we need to find the number of moles of hydrogen gas formed using the balanced chemical equation:
C + H2O -----> CO + H2
From the equation, we can see that for every 1 mole of carbon (C), we obtain 1 mole of hydrogen gas (H2). Therefore, 1.07 moles of C will produce 1.07 moles of H2.
Now, we can plug these values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
V = (1.07 mol * 0.0821 L.atm/mol.K * 315 K) / 1.0 atm
V = 27.329 L
Therefore, approximately 27.33 liters of hydrogen gas will be formed from the complete reaction of 1.07 moles of carbon (C), under the given conditions of 1.0 atm pressure and 315 K temperature.
To determine the volume of hydrogen gas formed, we can use the ideal gas law equation: PV = nRT. In this equation, P represents the pressure, V represents the volume, n represents the amount of substance in moles, R is the ideal gas constant, and T represents the temperature in Kelvin.
Given:
Pressure (P) = 1.0 atm
Temperature (T) = 315K
Amount of substance of C (n) = 1.07 mol
First, we need to find the number of moles of H2 formed in the reaction. By examining the balanced chemical equation, we can see that 1 mol of C produces 1 mol of H2. Therefore, the number of moles of H2 formed is also 1.07 mol.
Next, we rearrange the ideal gas law equation to solve for volume (V):
V = (nRT) / P
Substituting the known values:
V = (1.07 mol * 0.0821 L·atm/mol·K * 315K) / 1.0 atm
Now, we can calculate the volume of hydrogen gas formed:
V = (1.07 mol * 0.0821 L·atm/mol·K * 315K) / 1.0 atm
V ≈ 28.85 L
Therefore, approximately 28.85 liters of hydrogen gas will be formed from the complete reaction of 1.07 mol of C at a pressure of 1.0 atm and a temperature of 315K.
Use this example to calculate moles H2.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Then use PV = nRT to solve for volume.