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What must be the initial temperature of 22g of steam that is mixed with 90g of water at 68 degree celcius in an adiabatic calorimeter with a heat capacity of zero and that produces a mixture of 95g of water and 17g of steam at 100 degree celcius and 1atm?
Determine the mass of AgNO3 (MW = 170g/mol) required to dissolve in 400 mL solution in order to prepare a solution which is .14 M AgNO3.
The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produced 36.5 {rm g} of sodium upon decomposition. How much fluorine (in grams) was formed?
What mass of CaCO3 will produce 8.0 L of CO2, measured at standard temperature and pressure conditions? Molar mass of CaCO3 = 100. g per mole.
Methane and hydrogen sulfide form when 36g H2 texts with carbon disulfide. Calculate the percent yield if the actual yield of CH4 is 69.8g.
An unknown organic compound is mixed with 0.5190 g of naphthalene crystals to give a mixture having a total mass of 0.5959 g. The mixture is heated until the naphthalene melts and the unknown substance dissolves.
The EPA limit for lead in the water supply is 15 parts per billion by mass. Calculate the number of lead ions present in 1.00kg of water that is at the EPA limit for lead.
Calculate how many grams of Ni2+ are present in 3.36 moles of nickel(II) fluoride(NiF2) and also determine the number of moles of F- ion are present in 4.82 grams of nickel(II) fluoride.
The rate of a chemical reaction can sometimes be determined by measuring the change in mass of the reaction flask and its contents with time
A container holds 355 mL of a mixture of nitrogen and carbon dioxide gases. Calculate the partial pressures of each gas if the container is at 27.3oC.
Why are active firefighters likely to experience the adverse health effects from inhaling 300 ppm of carbon monoxide faster than nonactive off-duty firefighters
Explain why the atomic mass of an atom is a decimal number and how that value was determined before being placed on the periodic table.
Use the Frost Circle to draw the energy levels of the Pi molecular orbitals for this ion, show the electronic configuration and explain why the ion is aromatic.
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