Chemistry
posted by Neha .
92.01 grams of N2O4 (g) is placed in a container and allowed to dissociate.
N2O4 (g) > 2NO2 (g)
The mixture of N2O4 and NO2 resulting from the reaction occupies 36.0 liters
at a total pressure of 773 mmHg and 45 °C.
A. Let x equal the moles of N2O4 that dissociate. How many moles of N2O4
remain undissociated, and how many moles of NO2 are produced?
B. What are the mole fractions of N2O4 and NO2 in the mixture?
C. What are the partial pressures of N2O4 and NO2 in the mixture?

initial moles N2O4 = grams/molar mass = 92.01/92.01 = 1.00 moles.
.............N2O4 ==> 2NO2
initial.......1.0......0
change.........x......2x
equil.......1x........2x
and that answers #1. I don't know if you want a number or not but that can be obtained after you finish the rest of the problem.
B. Total moles = 1x+2x = 1+x
moles N2O4 = 1x
moles NO2 = 2x
XN2O4 = (1x)/(1+x)
XNO2 = 2x/(1+x)
Again, if a number is required, you can finish at the end.
C. PN2O4 = XN2O4*773/760
PNO2 = XNO2*773/760
Do you want numbers? If so, then use PV = nRT and solve for n. Using total volume, P, and T, you end up with total n. I solved this and came up with approximately 1.2 but you need to do it more accurately than that. Then you know total moles is 1+x from above. Since 1+x = 1.2, you can solve for x. Knowing x allows you to solve for mole fractions in B and partial pressure in C. 
VAPOUER DENSITY OF MIXTURE OF N2O4&NO2 is 38.3 at 25degree caliculate number of NO2 MOLICULES IN100 MOLES MIXTURE
Respond to this Question
Similar Questions

Chemistry
Calculate the rate at which N2O4 is formed in the following reaction at the moment in time when NO2 is being consumed at a rate of 0.0521 M/s. 2NO2(g) <> N2O4 (g) I am not really sure how to go about this problem. rate = k (N2O4) … 
chemistry
Kc=5.85x10^3 at 25 degrees C for the reaction N2O4(g)<>2NO2(g) fifteen(15.0) grams of N2O4 is confined in a 5.00L flask at 25 degrees C. Calculate(a) the number of moles of NO2 present at equilibrium and(b) the percentage … 
chemistry
Can you please check if I came up with the right answer for this please. A 4.30L container had 55.10 moles of N2O4 added to it. When equilibrium was established the concentration of N2O4 was found to be 1.69M.What is the Kc for the … 
chem
the total pressure of n2o4 and no2 IS 1.38 atm. if kp is 6.75(25 C) calculate partial pressure of NO2 in the mixture. 2NO2<> n2o4 
chemistry
The halflife for the firstorder decomposition of is 1.3*10^5. N2O4> 2NO2 If N2O4 is introduced into an evacuated flask at a pressure of 17.0 mmHg , how many seconds are required for the pressure of NO2 to reach 1.4mmHg ? 
Chemistry
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (g) > 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel initially containing .100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. … 
chemistry
A 1.00 mol sample of N2O4 (g) is placed in a 10.0 L vessel and allowed to reach equilibrium accourding to the equation N2O4(g) <> 2NO2(g) K = .0004 Calculate the equilibrium concentrations of N2O4(g) and NO2(g) 
chem 12
1.00 mol of N2O4 and 1.00 mol of NO2 are placed in an 800 mL container. Calculate the initial concentrations of each gas. N2O4= 1.25 mol/L NO2=1.25 mol/L When equilibrium is reached, the concentration of NO2 increases by 0.50mol/L. … 
chemistry
A reaction mixture of N2O4 and NO2 absorbs the heat given off in the combustion of 6.35 L CH4 measured at 24.7 C and 812 Torr. How many moles of N2O4 can be converted to NO2 as a result? 
Chemistry
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn=55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage …