Related Questions

A solid-oxide fuel cell is fed with carbon monoxide and reacts with air to produce CO2. This reaction will produce 2 electrons which are used to power an electric circuit external to the fuel cell. The reaction equation is shown below: 2CO(g) + O2(g) -> 2CO2(g) ΔHr° = -565.96 kJ/mol This reaction does not occur for other types of fuel cells which use a catalyst, such as polymerelectrolyte membrane or phosphoric-acid fuel cells. The presence of carbon monoxide on the anode side of these types of fuel cells will cause catalyst poisoning, reducing the efficiency and voltage of the fuel cell. Determine the rate of enthalpy change for a carbon dioxide production rate of 208 mol/hr. The extent of the reaction occurring in the fuel cell can be obtained by the following equation: where:
Refer to Q3, and estimate what is the total amount of heat (kcal) that must be removed by the cooling coil when this conversion is reached? Using the following equation: Q ̇= ΔHR r VR
Refer to Q3 and Q4 and estimate what is the maximum rate at which heat must be removed by the cooling coil (kcal/min) and at what time does this maximum occur? Using the following equation: Q ̇ = ΔHR kc2Ao VR
Calculate the ΔH of the following reaction: CO2(g) + H2(g)O -> H2CO3(g) if the standard values of ΔHf are as follows: CO2(g) : -393.509 KJ/mol, H2O(g): – 241.83 KJ/mol, and H2CO3(g) : – 275.2 KJ/mol.
ΔHf = V + ½ B + IEM – EAX + UL. What is V in this equation?
pure nickel melts at 1726K at 105 Pa (1 atm.) pressure, ΔV (solid-liquid) = 0.26 × 10-6 m3 . mol-1 and the heat of fusion, ΔHf = 18000 J.mol-1. The melting point of pure nickel, when acted upon by a pressure of 108 Pa is . . . . . . . . K.