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At 1478 oC the equilibrium constant for the reaction: 2 IBr(g) ? I2(g) + Br2(g) is KP = 0.899. If the initial pressure of IBr is 0.00169 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = . p(I2) = . p(Br2) = .
A sample of Nitrogen gas occupies 1.55L at 27.0 degrees C and 1.00 atm. What will the volume be at -100.0 degrees C and the same pressure?
calculate E when 830.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm.
burning 480 cm3 of propane measured at r.t.p,caused the temperture of 250 cm3 of water to increase by 42.5 celsius. calculate the heat of combustion of propane.
If a sample of 0.188 grams of KCN is treated with an excess of HCL, calculate the amount of HCN formed, in grams.
A sample of nitrogen occupies a volume of 250mL at 27 degrees C and 700 mmHg of pressure. What will be its volume at STP?
Garlic smell is easily noticable due to the compound that is responsible for this is Allicin , when we analysed this compaound and find out molecular formula of molar mass= 486 grams
It then gives off a photon having a wavelength of 1740 nm. What is the final state of the hydrogen atom? Values for physical constants can be found here.
The solution has a density of 1.286 g/cm3. Calculate E for the cell. Assume all the H+ ions come from the first dissociation of H2SO4, which is complete.
a compound contains 87.7% carbon and 14.3% hydrogen.its relative molecular mass is 70.what is the empirical formula and the molecular formula.and is it an alkane or alkene
Which of the following is a buffer?
weak base so you must consider other equilibria. (Ksp(ZnC2O4)=7.5X10^-9, Kb1=1.8X10^-10, Kb2=1.8X10^-13). Solve using systematic treatment of equilibrium.
Consider the malate dehydrogenase reaction from the citric acid cycle. Given the following concentrations, calculate the free energy change for this reaction at 37.0 °C (310 K).
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