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Calculate the amount of heat energy(q) gained when 150 g of water is heated from 25.0*C to 42.5*C.
Calculate the amount of heat energy (q) gained or lost when 180g of water is cooled from 65.0*C to 28.5*C. What is the sign of q for this calculation?
What is the % by mass of CaCl2.2H2O in the salt mixture B. how many grams of the excess reactant K2C2O4.H2O reacted in the mixture C. How many grams of the K2C2O4. H2O in the salt mixture remain unreacted
ultraviolet light strikes a metal plate and ejects electrons having kinetic energy E = 2.04 eV. Calculate the binding energy of an electron at the metal surface.
Identify the group of elements that corresponds to each of the following generalized electron configurations and indicate the number of unpaired electrons for each
0.134 mole of KCl and 0.185 mole of CaCl2 were dissolved in water. calculate the total number of moles of Cl- ions in the solution.
Solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of Hydrogen gas are formed when 48.7g of sodium are added to water?
A weather balloon at Earth's surface has a volume of 3.9 L at 275 K and 775 mm Hg. if the balloon is released volume reaches 4.2 L at 711 mm Hg what is the temperature.
how many grams of ice will still be present when the contents of the pitcher reach final temperaturethe tea is mostly water so assume that it has the same density (1g/mL), molar mass, heat capacity (75.3J/K/mol), and heat of fusion(6 kJ/mol) as pu..
A gas has a volume of 10 L at 0 degrees C. What is the final temperature of the gas in C if its volume increases to 27 L? Assume that amount of the gas and its pressure remain unchanged.
Calculate the amount of heat released when 5.3 moles of steam at 100 degrees celscus turns to water at the same temperature
A soluble salt, AgNO3, with a common ion is added to a saturated solution of AgCl to give [Ag^+]=2.0x10^-2 M. what is the [Cl^-]? AgCl Ksp=1.8x10^-10
The experimentally measured density under the same conditions is 3.10 g/L. Account for the discrepancy between your calculated value and the experimental result.
A liquid begins to appear on the inside of a closed flask. At first glance before the liquid began to appear, you might have thought the flask was empty
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