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The system CO2(g) + H2(g) *) H2O(g) + CO(g) is at equilibrium at some temperature. At equilibrium a 4.00 L vessel contains 1.00 mole CO2, 1.00 mole H2, 2.40 moles H2O, and 2.40 moles CO. How many moles of CO2 must be added to the system to bring the equilibrium CO concentration to 0.708 mol/L?
A tightly sealed 5.0 L flask contains argon at 69.0 deg. C and 781 mm Hg. The flask is heated until the pressure is doubled. What it the temperature of the gas.
Two compounds have the same empirical formula. One substance is a gas, the other is a viscous liquid. How is it possible for two substances with the same empirical formula to have markedly different properties?
Calculate the final temperature of the solution has a specific heat capacity =4.18 J/°C · g. assuming no heat lost
What mass of H2O is required to form 1.3L of O2 at a temperature of 320K and a pressure of 0.957atm.
calculate What mass of AlBr 3 is formed and calculate what mass of CCl 4 will be formed if 1.5 moles of CH 4 react with 1.4 moles of Cl?'
A flask contains 0.330 mol of liquid bromine, Br2. Determine the number of bromine molecules present in the flask.
How many kilograms of CO2 are produced from the complete combustion of 1.00L of gasoline assume that the gasoline has the formula C8H18.
Determine the value of the equilibrium constant at this temperature - Ammonium Hydrosulfide NH4HS yields NH3(Ammonia) and Hydrogen sulfide
A 115 mL sample of a 11.0 M ethylene glycol (rm C_2H_6O_2) solution is diluted to 1.40 L.What is the freezing point of the final solution? (Assume a density of 1.06 g/mL for the final solution.)
Determine the limiting reactant and also calculate how much of the gas is produced?
Compute the expected change in temperature for 1.7 grams of ammonium nitrate NH 4 NO 3 dissolved in 50.0 mili litres of water H 2 O.
How much heat is required to heat 10.0g of ice at -5.00 degree Celsius to become water vapor at 107.00 degree Celsius.
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