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Consider 25.0 g of water at 21.7°C that are mixed with 25.0 g of water at 43.3°C in a foam cup calorimeter. The equilibrium temperature reached was 30.4°C. Calculate the calorimeter constant in J/°C.
How much limestone must be decomposed by heating to produce 150.0 grams of lime, CaO?assuming that the limestone contains 85.0% pure CaCO3.
What is the volume of 290. mL of oxygen gas at 112°C and 790. mm Hg if the conditions are adjusted to STP? Assume the amount of gas is held constant.
The temperature is increased to 45 degree celcius then determine what is the pressure in the cylinder
2C4H10 + 13O2 → 8CO2 + 10H2O The equation shows the combustion of butane (C4H10). How many moles of water can be produced by 12.5 moles of C4H10 with excess oxygen.
2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g) + O2(g) If the initial concentration of NO is 0.150 M, what are the equilibrium concentrations of NO, N2, and O2.
if the density of mercury is 13.6g/cm3, what will be the volume of 300g of mercury ?
Compute the molar mass of the noble gas krypton(Kr) in a natural sample, which is 2.2% 80 Kr (molar mass 79.91 g/mol),
Is the reaction exothermic or endothermic? b) Calculate the heat produced when 10.0 g of AlCl3 forms. c) How many grams of Al are required to produce 1.00 kJ of energy?
Calculate the mass of nitrogen dissolved at room temperature in an 77.0 home aquarium. Assume a total pressure of 1.0 and a mole fraction for nitrogen of 0.78.
A piece of metal of mass 22 g at 92C is placed in a calorimeter containing 53.7 g of water at 21C. The final temperature of the mixture is 55.3C. What is the specific heat capacity of the metal?
Give the number of atoms of the specified element in a formula unit of each of the following compounds, and calculate the molecular (formula) mass
a 130g piece of metal is heated to 286C and dropped into 87.0g of water at 26C, if the final temperature of the water is 58.3C.
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