0.144 g of C60 is placed in a 100 cm3 container of hydrogen gas at a temperature of 20 °C and a pressure of 1.00 × 105 Pa.
The container is heated to make the C60 and hydrogen gas react. The reaction occurs as shown in the equation.
C60(s) + xH2(g) → C60H2x(s)
After the reaction, the container is allowed to cool to 20 °C. The pressure decreases to 2.21 × 104 Pa. All of the C60 has reacted.
i)
Name the type of reaction that occurs.
[1]
ii)
Calculate the amount, in moles, of C60 that reacts.
amount of C60 = .................................................... mol [1]
iii)
Calculate the amount, in moles, of hydrogen gas that reacted with the C60.
Show your working.
amount of hydrogen gas = .................................................... mol [3]
iv)
Use your answers from (c)(ii) and (c)(iii) to deduce the molecular formula of the hydrocarbon, C60H2x.
(If you were unable to calculate the amount of hydrogen gas, assume that 0.00240 mol of hydrogen gas reacts. This is not the correct value.)
Show your working.
molecular formula = ........................................................... [2]