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The molar heats of combustion of three hydrocarbon gases are:CH4 (methane)= - 890.0 kJ/molC2H6 (ethane)= - 1560.0 kJ/molC3H8 (propane)= - 2220.0 kJ/molFind the heat of combustion in kJ/g for each gas. These values are valid at 25°C, where the water produced by the reaction is in the liquid state.
What mimimum hydronium ion concentration (M) would be needed to prevent precipitation of cupric hydroxide (Cu(OH)2 Cu2+ + 2OH- , Ksp = 2.2 x 10-20) from a solution containing 0.010 M Cu2+ ion?
determine How many grams of AlCl 3 are formed if 30.0 grams of Hydrogen are produced? It is given that the molar mass of AlCl 3 =133.33 g/mol.
Calculating the rate of disappearance of HCl, The rate of disappearance of HCl was measured for the following reaction
Important information about Net ionic equation, What is the net ionic equation of 2Fe(NH4)2(SO4)2*6H2O + 6K2C2O4 + H2O2 + H2SO4
Calculate the pressure of a helium sample at -207.3°C and 768 mL if it exerts a pressure of 175 kPa at 25.0°C and 925 mL
All ammonium compounds, that comprise the ammonium ion (NH4+) and negative ion, are thermally unstable. Explain two ways that ammonium compounds decompose when they are heated.
Important information about Hydroboration reaction, In one experiment you combine 1-hexene which is reacted with H2SO4 with water as the solvent and the compound produced is 2-hexanol, and in another experiment you have 1-Methylcyclohexene
Do all chemical compounds undergo each type of chemical reaction,i.e. synthesis, decomposition, metathesis-precipitation, metathesis-neutralization, redox-single displacement, redox-combustion and can this information be useful to a criminal inves..
Hydrogen gas produced in the laboratory by the reaction of zinc and hydrochloric acid was collected over water at 25°C. The barometric pressure at the time was 742.5 mm Hg.
The feed to reactor contains only C 2 H 4 and HBr. if the molar flow rate = 165mol/s, compute the fractional conversion of the limiting reactant?
Determine the product of the reaction. As a general rule, a metal will combine with a nonmetal to form an ionic compound.
The tabulated mass of Cl is 35.45 amu. The two dominant isotopes of naturally occurring Cl are 35Cl (34.97 amu) and 37Cl (36.97 amu).
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