1. Consider a balloon filled with helium at the following conditions. 313 g He 1

Question

1. Consider a balloon filled with helium at the following conditions.

313 g He

1.00 atm

1910. L

Molar Heat Capacity = 20.8J/°C. mol

The temperature of this balloon is decreased by  as the volume decreases to , with the pressure remaining constant. Determine , , and  (in ) for the compression of the balloon.

2. the volume of a sample of an ideal gas (3.482g) was 754 ml at 1.98 atm and 62. the gas is

3. propane, CH, a hydrocarbon used in home heating/cooking, undergoes combustion to form gaseous CO and liquid HO; releasing -10,308K J in heat at 25°C.

write a balanced equation for the combustion of one mole of CH.

how many heat will be released when 22.047 g of propane is burned

313 g He

1.00 atm

1910. L

Molar Heat Capacity = 20.8J/°C. mol

Explanation / Answer

2)

mass of sample = 3.482 g

volume = 754 ml = 0.754 L

pressure = 1.98 atm

temperature = 62 + 273 = 335 K

PV = n RT

1.98 x 0.754 = n x 0.0821 x 335

n = 0.05428

moles = mass / molar mass of sample

molar mass of sample = 64 g/mol

so the gas is SO2

3)

C3H8 + 5 O2   -------------------> 3 CO2 + 4 H2O        heat = - 10.308 kJ

44.09        ---------------   heat = - 10.308 kJ

22.047    ---------------- ??

heat released = 22.047 x 10.308 / 44.09

                       = 5.15 kJ

heat released = - 5.15 kJ

Note : first question is not clear. what you want to determine

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