ok heres my question,

nitrogylcerin decomposes:

4c3h4(no5)3 --->12co2(g) +10h20(g)+6n2(g)+02(g)

whats is the max pressure that a 10.0L container will be able to withstand if 5.00 Nitroglycerin decomposes at temp of 1250c

mm of nitroglycerin =227 g/m

i got 2.00atm

b) what are the partial pressures

c02=.828
h20=.690
n2=.414
02=.0690

can u show me the method to do the total pressure. The rest i can do myself

thanks again

See the formula for nitroglycerin here.

Which formula is correct?http://en.wikipedia.org/wiki/Nitroglycerin

the formula is given

4c3h4(no5)3 --->12co2(g) +10h20(g)+6n2(g)+02(g)

Your equation isn't balanced. 16 H on the left (and you should try to capitalize those letters that need it) and I see 20 on the right. 60 O on the left and 36 on the right.

it was given so we don't have to. I think the teacher is just trying to show us how to use the mole ratios to get partial pressures

here this might help

4 C3H5(NO3)3(l) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)

I must have copied it wrong into the browser.

sorry...

To calculate the maximum pressure a 10.0L container can withstand when 5.00g of nitroglycerin decomposes at a temperature of 1250°C, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin

Let's break this down step by step:

Step 1: Convert the temperature to Kelvin
T (in Kelvin) = 1250°C + 273.15 = 1523.15 K

Step 2: Calculate the number of moles of nitroglycerin used
Given that the molar mass of nitroglycerin (MM) is 227 g/mol and we have 5.00g of nitroglycerin:
Number of moles of nitroglycerin = mass / molar mass
Number of moles = 5.00g / 227 g/mol

Step 3: Use the balanced equation to find the ratio of the moles of nitroglycerin to the number of moles of gases produced
From the balanced equation:
1 mole of nitroglycerin produces 12 moles of CO2
1 mole of nitroglycerin produces 10 moles of H2O
1 mole of nitroglycerin produces 6 moles of N2
1 mole of nitroglycerin produces 1 mole of O2
So, the ratio is:
12 moles of CO2 : 10 moles of H2O : 6 moles of N2 : 1 mole of O2

Step 4: Calculate the moles of each gas produced
Moles of CO2 = (Number of moles of nitroglycerin) x (12 moles CO2 / 1 mole nitroglycerin)
Moles of H2O = (Number of moles of nitroglycerin) x (10 moles H2O / 1 mole nitroglycerin)
Moles of N2 = (Number of moles of nitroglycerin) x (6 moles N2 / 1 mole nitroglycerin)
Moles of O2 = (Number of moles of nitroglycerin) x (1 mole O2 / 1 mole nitroglycerin)

Step 5: Calculate the partial pressures of each gas
Partial pressure = (moles of the gas) x (R) x (temperature in Kelvin) / (volume of the container)

Partial pressure of CO2 = (moles of CO2) x (R) x (temperature in Kelvin) / (volume of the container)
Partial pressure of H2O = (moles of H2O) x (R) x (temperature in Kelvin) / (volume of the container)
Partial pressure of N2 = (moles of N2) x (R) x (temperature in Kelvin) / (volume of the container)
Partial pressure of O2 = (moles of O2) x (R) x (temperature in Kelvin) / (volume of the container)

Step 6: Calculate the total pressure
Total pressure = sum of all partial pressures

By plugging in the appropriate values and calculating, you will find the max pressure a 10.0L container can withstand and the individual partial pressures of each gas.