Question

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?

Answer 1

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.

Answer 2

calculate the delta h of 3.1g of magnesium and 10g of HCL