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Carbon Monoxide(0.40mol) and water(0.4 mol) are placed in a 2.0 vessel and are allowed to reach equilibirum at 100 degrees celsius.where the equilibrium constant k= 0.58. Calculate the equilibrium concentrations of the 4 gases: Equation: CO(g)+H2O(g)=> CO2(g)+H2(g) Kc=0.58@100degrees Celsius Using the ICE table might help but I have trouble with that alot
Calculate the pH and pOH of each of the following solutions. [H3O+] = 1.5x10^-8 M? [H3O+] = 1.0x10^-7 M? [H3O+] = 2.2x10^-6 M
The partial pressure of oxygen gas in an atmosphere at STP is approximately 0.2 atm. If I capture 11.2 liters of atmospheric gas at STP in a flask,
If a 1.00g sample of a carbon-containing compound is burned in air, 0.75g of CO2(the only carbon-containing product) is produced. What is the mass% carbon in the compound
How many moles of iron atoms are in 2.28 mol of Fe2O3?
the chloroform would remain as liquid in the flask after equilibrium is established between liquid and vapor chloroform? (the vapor pressure of chloroform at 20 degrees C is 0.208 atm)
When an ice cube is dropped into a Styrofoam cup containing 195 g of coffee at 97.0 oC, the thermal energy used to melt the ice is 2.1 kJ what is the final temperature of the coffee closest to ? (Assume a specific heat of 4.184 J/g oC for the coff..
If a bottle of nail polish remover contains 172 of acetone,how much heat would be released by its complete combustion? The density of acetone is 0.788 .
What volume of H2 (at 25oC and 1.00 atm ) can be produced by reaction of 161 g Fe and 202 g of HCl? (Atomic weights: Fe = 55.85, Cl = 35.45, H = 1.008)
The equation for the combustion of gaseous methanol is: 2CH3OH(g) + 3O2(g) ? 2CO2(g) + 4H2O(g) Estimate the ?H°rxn per mole of methanol combusted, using the bond energy data provided below
A 20.00mL sample of H3Y was titrated with 0.1000 M NaOH. The first equivalence point was reached after the addition of 14.98mL of base. The second equivalence point was reached after the addition of 30.03mL.
The reaction 2NO (g)-> N2 (g) + O2 (g) has a H = 180.5 kJ. How much heat will be required to produce 44.8 L of NO by the reverse reaction?
The enthalpy of formation of compound X is -612 kJ/mol, and the sole product of its combustion has a enthalpy of formation of -671 kJ/mol. What is the enthalpy of combustion of compound X?
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