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A large tank contains 1000 moles of air at 525 degrees celsius. Air is drawn out of this tank at 10 moles/s and replaced with ambient air at 25 degrees celsius. Assume air in tank is mixed and that air is an ideal diatomic gas. For a heated tank what heat rate must be applied to keep the tank air temperature constant? For a perfectly insulated tank, what is the tank air temperature after 100 seconds? The pressure in the tank is not given, explain why it is not needed?
There are two ways of utilizing hydrogen as fuel in automobiles - as the replacement of gasoline in internal combustion engine or in a fuel cell. Can you explain why a fuel cell is more efficient using the Second Law of Thermodynamics
Container A holds 727 mL of ideal gas at 2.20 atm. Container B holds 134 mL of ideal gas at 4.20 atm. If the gases are allowed to mix together
Compute the reactor volume and space time to get 90% conversion in a PFR and in a CSTR
What is the pressure (in atmospheres) of a sample of gas trapped in the closed-tube mercury manometer
A solution is prepared by adding 60.0 mL of 0.060 M HBr to 180.0 mL of 0.70 M HI. Calculate the concentrations of all species in this solution. HBr and HI are both considered strong acids
When 9.25 g of ClF3 was introduced into an empty 2.00 L container at 700.0 K, 19.8 % of the ClF3 decomposed to give an equilibrium mixture of ClF3, ClF, and F2.
Calculate the amount of heat trasnferred when 3.55 g of Mg(s) reacts at constant pressure. 2Mg(s) + 02(g) ---> 2MgO(s) heat= -1204kJ
Estimate how many barrels of fluid this tank could hold. Clearly state any assumption you must make to determine this and explain how you arrived at your assumption
What is the amount of volume of the solvent you need to extract 65g of the solute in one extraction from the original 100g dissolved in 206mL water?
Determine the pressure of a gas using the ideal gas law - Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.
Since you need pressure based constant use ideal gas equation (PV=nRT) to convert moles of gas into pressure with units of atmospheres. R=0.0821 L atm/mol K
How many moles of carbon monoxide react with 1 mole of oxygen gas according to the balanced chemical equation?
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