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Problem- Top fuel dragsters and funny cars burn nitromethane as fuel according to the following balanced combustion equation:
2CH3NO2(l)+3/2O2(g)?2CO2(g)+3H2O(l)+N2(g)
The standard enthalpy of combustion for nitromethane is ?1418kJ.
Calculate the standard enthalpy of formation (?H?f) for nitromethane.
Mention step wise computation of your work done
Hydrogen bromide can be prepared by the reaction of hydrogen gas and bromine gas as per the equation shown below (H2 (g) + Br2 (g) → 2HBr (g). Whas mass of product will be obtained when 1.34 mol of bromine gas is used in the reaction
Estimate the boiling point elevation of a saturated solution of LiF at 100 degrees Celsius, assuming it undergoes complete dissociation. The solubility of LiF is 230 mg/100 g of water at 100 degrees celsius, and the boiling point constant of water..
150g sample of a pure compound subjected to catalytic hydrogenation takes up 25.0mL of H2 at 25 degrees Celsius and 1atm pressure. Compute the molecular weight of the compound presume that it has only one double bond.
How many grams of NaF form when 0.580 mol of HF reacts with excess Na2SiO3?
Aluminum has chemical propertied that are similar to magnesium. What observation might you expect with the addition of 6M HCl
Calculate the densities of of each of the following gases in g/L at ATP: a) C3H8; b) NH3; c) Cl2; d) Ar.
a strip of electrolytically pure copper weighing 3.178 gram is strongly heated in a stream of oxygen until it is all
Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2. 2 C8H18 + 25 O2 ? 16 CO2 + 18 H2O
The acid-dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.2 × 10-13 at 25.0 °C. What is the pH of a 2.5 M aqueous solution of phosphoric acid
X reacts with one molar equivalent of hydrogen in the presence of a palladium catalyst to form 1,2-dimethylcyclopentane. Treatment of X with ozone follwed by zinc in aqueous acid gives a dialdehyde.
An aqueous solution of CaCl2 has a vapor pressure of 84.0mmHg at 50 C . The vapor pressure of pure water at this temperature is 92.6mmHg . What is the concentration of CaCl2 in mass percent?
How much work would have been done if the gas were ideal? Account for the differences the two values.
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