What volume of nitrogen at 215 degress celcius and 715 mmHg would be required to react with .100 moles of hydrogen to produce ammonia?
N2+3H2--> 2NH3
If the H2 is at the same T and P as the N2, then you need not correct for the P and T not being at STP.
100 mol H2 x (1 mol N2/3 mol H2) = 100 x 1/3 = ?
To determine the volume of nitrogen required to react with 0.100 moles of hydrogen, we can use the stoichiometry of the balanced chemical equation.
The balanced chemical equation is:
N2 + 3H2 → 2NH3
From the equation, we can see that one mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3.
First, let's convert the number of moles of H2 to moles of N2 using the ratio of its coefficients.
Moles of N2 = 0.100 moles of H2 × (1 mole N2 / 3 moles H2)
Moles of N2 = 0.0333 moles of N2
Now, we can use the ideal gas law to calculate the volume of nitrogen at the given temperature and pressure.
The ideal gas law equation is:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
Let's convert the given temperature from Celsius to Kelvin.
T(K) = 215°C + 273.15
T(K) = 488.15 K
Now, we can rearrange the ideal gas law equation to solve for V.
V = (nRT) / P
Substituting the given values:
V = (0.0333 moles × 0.0821 L·atm/(mol·K) × 488.15 K) / (715 mmHg × 1 atm / 760 mmHg)
Simplifying the equation:
V = (0.0333 moles × 0.0821 L·atm/(mol·K) × 488.15 K) / (715 × 760)
Calculating the volume:
V ≈ 0.704 L
Therefore, approximately 0.704 liters of nitrogen gas would be required to react with 0.100 moles of hydrogen to produce ammonia.
To answer this question, we need to use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, let's gather the given information:
- Moles of hydrogen (H2) = 0.100 moles
- Temperature (T) = 215 degrees Celsius, which needs to be converted to Kelvin. To do this, we add 273 to the Celsius temperature:
T = 215 + 273 = 488 Kelvin
- Pressure (P) = 715 mmHg, but we need to convert it to atm because the ideal gas constant is in atm:
1 atm = 760 mmHg
P = 715 mmHg ÷ 760 mmHg/atm = 0.94 atm
Next, we need to calculate the number of moles of nitrogen (N2) needed to react with the given moles of hydrogen (H2). From the balanced chemical equation, we know that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia (NH3). Therefore, we can use a mole ratio:
0.100 moles H2 × (1 mole N2 / 3 moles H2) = 0.0333 moles N2
Now, we can plug in the values in the Ideal Gas Law equation to calculate the volume of nitrogen (V):
PV = nRT
V = (nRT) / P
V = (0.0333 moles × 0.0821 L·atm/(mol·K) × 488 K) / 0.94 atm
V ≈ 1.69 L
Therefore, approximately 1.69 liters of nitrogen would be required to react with 0.100 moles of hydrogen to produce ammonia at a temperature of 215 degrees Celsius and a pressure of 715 mmHg.