Question 15
2 Points
How much energy is required to heat 44.72 g of H2O from 10.00 oC to 37.50 oC? (Heat capacity of liquid H2O = 75.37 J mol-1 K-1) (type in the numeric value in Joules - give your answer to 4 significant figures, do not include the units in your answer only the number, do not use scientific notation, do not include comma's) BLANK-1
temperature difference is same
in °C as well as in Kelvin so do not bother to convert the
unit.
Question 15 2 Points How much energy is required to heat 44.72 g of H2O from...
Question 16 8 Points Silver is known to be an excellent conductor of heat and electricity. if 8.20 kJ of energy are provided, calculate the energy required (Joules - just put in the number, 4 sig figs) to heat 14.25 g of silver from 25.00 °C to its melting point BLANK-1, the energy required (kJ - just put in the number, 4 sig figs) to melt the silver BLANK-2, and determine whether the silver will reach the boiling point. (yes/no)...
1. At 1 atm, how much energy is required to heat 35.0 g H2O(s) at −10.0 ∘C to H2O(g) at 137.0 ∘C? Use the heat transfer constants found in this Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000...
At 1 atm, how much energy is required to heat 43.0 g H2O(s)43.0 g H2O(s) at −14.0 ∘C−14.0 ∘C to H2O(g)H2O(g) at 121.0 ∘C?121.0 ∘C? Use the heat transfer constants found in this table. Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O...
At 1 atm, how much energy is required to heat 73.0 g H2O(s)73.0 g H2O(s) at −14.0 ∘C−14.0 ∘C to H2O(g)H2O(g) at 159.0 ∘C?159.0 ∘C? Use the heat transfer constants found in this table. Heat-transfer constants for H2O at 1 atm Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C)...
At 1 atm, how much energy is required to heat 75.0 g of H2O(s) at –22.0 °C to H2O(g) at 145.0 °C? Helpful constants can be found here. Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000 J/(g·°C) *...
At 1 atm, how much energy is required to heat 81.0 g of H2O(s) at –20.0 °C to H2O(g) at 149.0 °C? Helpful constants can be found here. These are the helpful constants: Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous...
How much energy is required to heat 36.0 g H2O from a liquid at 55.0°C to a gas at 150.0°C? The following physical data may be useful. Molar Mass(H2O) = 18.0 g/mol ΔHvap = 40.7 kJ/mol Cs;liquid = 4.18 J/g oC Cs;gas = 2.01 J/goC Tb(H2O) = 100.0 oC
Calculate the quantity of heat energy, in Joules, that is absorbed when a gold (.128J/goC) ring with a mass of 12.68 is warmed from 23.2 oC to 58.1 oC. Report your answer, in J, using the correct number of significant figures. Do not enter units and do not use scientific notation.
Question 19 3 Points Smelling salts work by releasing ammonia to the reaction (NH4)2CO3 (s) --> 2 NH3 (g) + CO2 (g) + H2O (l) Use Hess' law to calculate the heat of reaction (in kJ) BLANK-1 (Give your answer to 3 significant figures, do not include units in your answer, do not use scientific notation) ΔHof {(NH4)2CO3)} = +156 kJ/mol, ΔH0f {NH3} = -46.1 kJ/mol, ΔH0f {CO2} = -393.5 kJ/mol, ΔH0f {H2O}= -285.8 kJ/mol BLANK-1
A. How much heat energy, in kilojoules, is required to convert 68.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to three significant figures and include the appropriate units. B. How long would it take for 1.50 mol of water at 100.0 ∘C to be converted completely into steam if heat were added at a constant rate of 17.0 J/s ? Express your answer to three significant figures and include the appropriate units.