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What is the boiling point of the automobile radiator fluid prepared by mixing 1.00 L of ethylene glycol (HOCH2CH2OH, density - 1.114 g/mL) with 1.16 L of water (density = 1.000 g/mL)? The Kb of water is 0.52 degrees C/m.
During a strenous workout, an athlete generates 1890.0 kj of heat energy. What mass of water would have to evaporate from the athlete's skin to dissipate this much heat?
what is the volume of the hydrogen gas (at25oC and 100KPA) needed to produce 51.1g of ammonia?
What is the molarity of aqueous silver nitrate if 50.00 mL of AgNO3 reacts with 25.0 mL of 0.100
Assuming the solution has a heat capacity of 4.18 J/°C·g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Calculate the fraction of atom sites that are vacant for silver at 695°C. Assume an energy for vacancy formation
The most common source of copper is the mineral chalcopyrite (CuFeS2) how many kilograms of chalcopyrite must be mined to obtain a 440 grams of pure copper.
Exact potential difference in the concentration cell, What will be the exact potential difference in the following concentration cells?
Calculate the pH of the 0.20 M NH3/0.24 M NH4Cl buffer. B)What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 55.0 mL of the buffer?
How much heat is required to warm 229 g of ice from -44.7°C to 0.0°C, melt the ice, warm the water from 0.0°C to 100.0°C, boil the water, and heat the steam to 173.0°C?
If 145 grams of potassium nitrate were added to water to make 1,500 mL of solution, what would be the molarity of the resulting solution?
Consider the reaction Cu2S + O2 → 2Cu + SO2. If 55.0 grams of Cu2S is heated in excess O2, what is the mass of Cu that can be produced?
Calculate the empirical and molecular formulae of A and B. Deduce the structural formulae of A and B. State the type isoerism exhibited by A and B.
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