Calculate the volume of carbon dioxide at room temperature and pressure that can beobtained from 30.0 g of glucose.......................... dm3 [1](c) Ethanol can also be manufactured from ethene.(i) Name the raw material which is the source of ethene........................................................................................................................................ [1](ii) Write a balanced equation for the manufacture of ethanol from ethene........................................................................................................................................ [1][Total: 9]PhysicsAndMathsTutor.com

To answer your question, we need to break it down into several parts:

1. Calculate the volume of carbon dioxide at room temperature and pressure that can be obtained from 30.0 g of glucose:

The balanced equation for the combustion of glucose is C6H12O6 + 6O2 -> 6CO2 + 6H2O. From this equation, we can see that one mole of glucose produces six moles of carbon dioxide.

The molar mass of glucose (C6H12O6) is approximately 180 g/mol. So, 30.0 g of glucose is 30.0 g / 180 g/mol = 0.167 mol.

Since one mole of glucose produces six moles of carbon dioxide, 0.167 mol of glucose will produce 0.167 mol * 6 = 1.002 mol of CO2.

At room temperature and pressure (RTP), one mole of any gas occupies 24.0 dm3. Therefore, the volume of CO2 produced is 1.002 mol * 24.0 dm3/mol = 24.048 dm3.

2. Ethanol can also be manufactured from ethene:

(i) The raw material which is the source of ethene is petroleum.

(ii) The balanced equation for the manufacture of ethanol from ethene is C2H4 + H2O -> C2H5OH.