5.95 g of Al reacts with sulphuric acid to form aluminum sulphate solution and hydrogen gas. What volume of hydrogen gas would be produced at T degree Celsius and 300 KPa?....

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justaguide | College Teacher | (Level 2) Distinguished Educator

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The amount of a gas in moles (n), the temperature (T) and the pressure (P) it is at is related to the volume (V) of the gas by the relation P*V = n*R*T where R is a constant equal to 8.314L*k*Pa/(K*mol)

When aluminum reacts with sulphuric acid, the reaction that takes place is `2Al + 3H_2SO_4 -> Al_2(SO_4)_3 + 3H_2` . For each mole of aluminum 1.5 moles of hydrogen is generated.

The molar mass of aluminum is 27, 5.95 g of Al is equivalent to approximately 0.22 moles. When the aluminum reacts, 0.33 moles of hydrogen is released. Using the ideal gas law the volume of 0.33 moles of hydrogen at a temperature T (in kelvin) is:

V = (n*R*T)/P = (0.33*8.314*T)/300 `~~` 9.14*T liters.

The volume of the hydrogen produced is approximately 9.14*T liters.

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