How is graphite different from other allotropes of carbon? a. graphite forms only from carbon atoms, without other atoms mixed in. b. the carbon atoms in graphite are arranged randomly, without a crystalline structure. c. the carbon atoms in graphite are arranged in widely spaced layers. d. the carbon atoms in graphite are packed extremely densely and tightly.

C. The carbon atoms in graphite are arranged in widely spaced layers.

Explanation:

Allotropes are different structural forms of the same element that exist is the same physical state. In other words, they differ in their bonding arrangement.

Carbon has two allotropes: diamond and graphite.

In diamond each C atom is sp3 hybridised and is bonded to 4 other C atoms forming a tetrahedral unit which extends into a crystalline network. In contrast, each C atom in graphite is sp2 hybridised and bonded to 3 other carbon atoms in a crystalline hexagonal layer like structure.

Thus, the carbon atoms in graphite are arranged in widely spaced layers.

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :