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The standard enthalpy of formation of NH3(g) is -46.0 kJ/mol. Calculate the thermal energy evolved when 8.0g of H2(g) react with an excess of N2(g).
The solid copper (II) carbonate was isolated by vacuum filtration and dried; 0.920 g of copper (II) carbonate was collected. The net ionic equations for the reactions which occurred are shown below.
What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass. HCO
Calculate the mass of urea that should be dissolved in 225 g of water at 35°C to produce a solution with a vapor pressure of 37.1 mmHg.
Calculate moles of permanganate required. b. Show a balanced redox equation i. oxidation ii. reduction iii. overall c. How many moles of lead are present
ammonia reacts with diatomic oxygen to form nitric oxide and watervapor. when 40.0g of ammonia and 50.0 g of oxygen
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.
Write the balanced formula unit equation for the reaction of hydrobromic acid with magnesium hydroxide. What is the sum of the coefficients?
benzene is a hydrocarbon that is commonlynbsp used as a commercial solvent. however it isnbsp carcinogenic i.e.
Identify the elements that correspond to the following atomic numbers. label each as a noble gas ? a halogen ?an alkali metal? an alkaline earth metal? a transition metal? a lanthanide metal? or an actinide metala 17 b 4 c 63 d 72 e 2 f 92 g 55
state three disadvantages of the wittig
Assume that you are an experienced organic chemist with perfect recrystallization technique. You recrystallize 10g of impure naphthalene from Ethanol in Corvallis, OR (elevation; sea level) and recover 7.4g of pure naphthalene.
The fuel used in many disposable lighters is liquid butane, C4H10. How many carbon atoms are in 2.00 g of butane
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