Given the following at 25degreeC and 1.00 atm: 1/2 N2(g) + O2(g) rightarrow NO2(

Question

Given the following at 25degreeC and 1.00 atm: 1/2 N2(g) + O2(g) rightarrow NO2(g) Delta H degree +33.2 kJ N2(g) + 2 O2(g) rightarrow N2O4(g) Delta H degree +11.1 kJ Calculate the Delta H degree for the reaction below at 25degreeC.2NO2(g)rightarrow N2O4(g) An experiment shows that a 389.0 mL gas sample has a mass of 0.2360 g at a pressure of 0.9380 atm and a temperature of 302.15 K. What is the molar mass of the gas? Assuming it behaves as an Ideal gas, what is the density of 1.00 mol of H2 gas at a pressure of 2.34 atm and a temperature of 300.00 K?

Explanation / Answer

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1.

2 x Reaction 1 + final Reaction = 2 x Reaction 2

Final Reaction = 2(R2 – R1)

dH = 2x(11.1 – 33.2) = - 44.2 kJ

2.

pV = nRT

pV = (m/M) RT

M = mRT/(pV)

     = 0.2360 g x 0.0821 L.atm.K1 mol1 x 320.15 K /(0.9380 atm x 0.389 L) =

     = 17.000 g/mol

3.

d= m/V

m/V = pM/(RT)

d = 2.34 atm x 2 g/mol / (0.0821 L.atm.K1 mol1 x 300 K) = … g/L

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