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A standard blue dye solution is labeled 427ppm. The dye in the solution has a molar mass of 412g/mol. The solution is diluted by taking a 5.00mL sample, adding it to a 25.00mL volumetric flask and diluting to the mark with water. Calculate the new concentration and give the value in units of molarity.
what is the mass of the solid nh4cl formed when 64.0 g of nh3 are mixed with an equal mass of hcl? what is the volume
how many electrons are gained or lost by each sulfur atom. how many electrons are gained or lost by each copper atom
Problem- If 0.0280 mol of CaCl2 is dissolved in water to make a 0.710 M solution, what is the volume of the solution?
Estimate the amount of heat released (in kj/mol) when 10g of CH4 gas reacts with an excess of O2 gas to form gaseous CO2 and liquid water. The molar mass of CH4 is 16.042.
an equilibrium mixture of so2 o2 and so3 at a high temperature contains the gases at the following concentrations so2
a solution is 40 acetic acid by mass. the density of this solution is 1.049 gml. calculate the mass of pure acetic acid
Problem- A gaseous mixture contains 25.3% methane, 38.2% ethane and the rest is propane by volume. When the fuel mixture contained in a 1.55-L tank, stored at 755 torr and 298 K, undergoes complete combustion, how much hear is emitted
for a hydrogen atom calculate the energy of a photon in the balmer series that results from the transition n 3 to n
State a mechanism for the dehydration of 4-methylcyclohexanol catalyzed by an acid? In the case utilize H3PO4 and a little bit of H2SO4 plus heat. The products are 4-methylcyclohexene + H20.
Give the term symbol for the term occurs from each of the subsequent H-atom electron configurations, 1s, 2p, 3d. Give the values for L and S for a 4F term
Car batteries are filled with sulfuric acid. What is the mass of the acid (in grams) in 500.0 mL of the battery acid solution if the density of the solution is 1.285 g/cm^3 and if the solution is 38.1% sulfuric acid by mass.
Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6(l) + 15 O2(g) ? 12 CO2(g) + 6 H2O(g) ?H°rxn = -6278 kJ
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