NH4NO3(s) H2O(g) + N2(g) + O2(g)
Consider the unbalanced equation above.
What will be the total volume of gas produced at 720. mm Hg and 570.0°C when 2.50 g of NH4NO3 completely decomposes? Use molar masses with at least as many significant figures as the data given.
You don't have an equation because you don't have an arrow. And I can't figure out where the arrow goes. When you do, here is a link that will get you through the remainder of the problem. This link is an example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To find the total volume of gas produced, we need to balance the equation and determine the number of moles of gas produced.
First, let's balance the equation:
NH4NO3(s) -> H2O(g) + N2(g) + O2(g)
The coefficient in front of NH4NO3 is already 1. So, let's balance the nitrogen (N) atoms by placing a coefficient of 2 in front of NH4NO3:
2 NH4NO3(s) -> H2O(g) + N2(g) + O2(g)
Now, let's calculate the number of moles of NH4NO3 using its molar mass. The molar mass of NH4NO3 is:
NH4NO3 = 1(14.01 g/mol) + 4(1.01 g/mol) + 3(16.00 g/mol) = 80.04 g/mol
Number of moles of NH4NO3 = mass / molar mass = 2.50 g / 80.04 g/mol
Next, we need to use stoichiometry to find the number of moles of gas produced from the balanced equation. Looking at the coefficients in the balanced equation, we can see that 2 moles of NH4NO3 produce 1 mole of N2 and 2 moles of NH4NO3 produce 1 mole of O2.
From the calculated number of moles of NH4NO3, we can determine the moles of N2 and O2 produced as follows:
moles of N2 = (2.50 g / 80.04 g/mol) * (1 mol N2 / 2 mol NH4NO3)
moles of O2 = (2.50 g / 80.04 g/mol) * (1 mol O2 / 2 mol NH4NO3)
Now, we can use the ideal gas law to calculate the total volume of gas produced.
The ideal gas law is expressed as:
PV = nRT
Where:
P is the pressure (720 mmHg)
V is the volume (unknown, what we want to find)
n is the number of moles of gas (moles of N2 + moles of O2)
R is the ideal gas constant (0.0821 L * atm / (K * mol))
T is the temperature in Kelvin (570.0°C + 273.15)
Rearranging the equation to solve for V, we have:
V = (nRT) / P
Substituting the values into the equation, we can calculate the total volume of gas produced.