Reactants for the following reaction are placed in a 10.0 L flask held at 250 degrees C and at initial partial pressures of 1.00 atm each. Calculate the final pressures of each reactant and product, assuming the reaction goes to completion. 4 N2O(g) + CH4(g) = 4N2(g) + 2H2O(g). What is the final pressure in atmospheres?
Use PV = nRT to calculate moles N2O.
Use PV = nRT to calculate moles CH4.
Using the coefficients in the balanced equation, determine the limiting reagent.
Convert moles reactants, with regard to the limiting reagent, to moles of the products. Then use PV = nRT to calculate partial pressure of each gas. The sum of partial pressures will be the total pressure.
NOTE: Be aware that if you have a limiting reagent that there will be some of the non-limiting reagent material not used. You will be required to calculate the moles not used in the reaction and include a calculation for partial pressure of that gas and add it into the total pressure. Post your work if you get stuck.
calculate the delta h of 3.1g of magnesium and 10g of HCL
To calculate the final pressures of each reactant and product, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas
V = volume of the flask
n = number of moles of the gas
R = ideal gas constant (0.0821 atm L/mol K)
T = temperature in Kelvin
First, we need to calculate the number of moles for each reactant and product using the given initial partial pressures and the volume of the flask.
1. Convert the temperature to Kelvin:
T = 250 degrees C + 273.15 = 523.15 K
2. Calculate the number of moles of CH4:
n_CH4 = (P_CH4 * V) / (R * T)
= (1.00 atm * 10.0 L) / (0.0821 atm L/mol K * 523.15 K)
3. Calculate the number of moles of N2O:
n_N2O = (P_N2O * V) / (R * T)
= (1.00 atm * 10.0 L) / (0.0821 atm L/mol K * 523.15 K)
4. Calculate the final number of moles of N2:
n_N2 = 4 * n_N2O
5. Calculate the final number of moles of H2O:
n_H2O = 2 * n_N2O
Now that we have the number of moles for each reactant and product, we can calculate their final pressures.
6. Calculate the final pressure of CH4:
P_CH4_final = (n_CH4 * R * T) / V
7. Calculate the final pressure of N2O:
P_N2O_final = (n_N2O * R * T) / V
8. Calculate the final pressure of N2:
P_N2_final = (n_N2 * R * T) / V
9. Calculate the final pressure of H2O:
P_H2O_final = (n_H2O * R * T) / V
Finally, to find the final pressure in atmospheres, you can add up the final pressures of all the gases:
Final pressure = P_CH4_final + P_N2O_final + P_N2_final + P_H2O_final
Just substitute the values calculated in steps 6-9 into the final pressure equation to get the answer.