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Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g) with K = 1.6 x 10-5 1.00 mole of pure NOCl and 1.00 mole of pure Cl2 are placed in a 1.00-L container. If x moles of NOCl react, what is the equilibrium concentration of Cl2? Why is the answer C) 1 + x/2
A 14.0 g sample of X combines with a 26.2 g sample of Y to form the compound XY2. What is the mass of the reactants.
Consider: C7H16 (l) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (l) ΔH°reaction=- 4130 kJ. How much energy is released when 4.000 moles of C7H16, is combusted?
A 44 sample of water absorbs 329 of heat If the water was initially at 21.7, what is its final temperature.
Calculate the amount of 10.00% acetic acid you will need to add to 100.0 mL of your milk in order to bring the final acidity to 1.00% acetic acid.
A 355 m-L container holds .146 g of Ne and an unknown amount of Ar at 35 degrees C and a total pressure of 626 mmHg. Calculate the moles of Ar present.
For the equation: C (s) + CO2 (g) -> 2CO (g); the value of Kp is 167.5 at 1000 oC. If a 5.00 L container initially contains 2.99 atm pressure of CO2 (g) at 1000 oC, what are partial pressure of CO2 (g) and CO (g) at equilibrium?
If 6.06 L of O2 gas is collected over water at 250C (vapor pressure = 23.8 torr) and a barometric pressure of 702 torr, what is the mass of H2O2 (MM = 34.02 g/mole) decomposed?
Alkenes contain double bonds while alkynes contain triple bonds, Naming compounds containing double as well as triple bonds
477 J amount Energy is added to a 74.0 grams sample of H 2 O at a temperature of 21 degree Celsius. Determine what will be the final temperature of the H 2 O?
What you need to know about Problems, The Ksp of La(IO3)3 is 1.0×10-11. Using activities, what is the molar solubility of La(IO3)3 in a 0.050 M solution of NaNO3?
The average pH of precipitation in rural areas is 5.80. Assuming that the pH is controlled by the carbonate system, i.e., no anthropogenic acid gases are present in the atmosphere.
An electric power station annually burns 3.3 107 kg of coal containing 1.4 percent sulfur by mass. Calculate the volume of SO2 emitted at STP
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