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22:02 4 Exit Question 8 4 pts ice A piece of aluminum lost 100.0 J of...
Calculate the amount of heat in J required to increase the temperature of 25.0 grams of...
Calculate the amount of heat in J required to increase the temperature of 25.0 grams of water from 25. °C to 50.0 °C. ice Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol Specific Heat (J/g (state) °C) helium He(s) 5.193 water H2O(1) 4.184 ethanol C2H60(1) 2.376 H2O(s) 2.093 (at -10 °C) water vapor H2O(g) 1.864 nitrogen N2(8) 1.040 air 1.007 oxygen O2(8) 0.918 aluminum Al(s) 0.897 carbon CO2(8) 0.853 dioxide argon Ar(s) 0.522 iron Fe(s)...
Which of the following (with specific heat capacity provided) would require the least energy to increase...
Which of the following (with specific heat capacity provided) would require the least energy to increase temperature by 1 oC? 1.0 g H2O(g) (Cs = 1.864 J/g oC) 1.0 g Si(s) (Cs = 0.712 J/g oC) 1.0 g O2(g) (Cs = 0.918 J/g oC) 1.0 g Pb(s) (Cs = 0.130 J/g oC) 1.0 g Al(s) (Cs = 0.897 J/g oC)
the Specific Heat Capicity of Tungsten is given here. 3. Calculate the temperature change when 32...
the Specific Heat Capicity of Tungsten is given here.
3. Calculate the temperature change when 32 grams of tungsten has 21 Joules of heat added to it. temperature be- in between the initial temperatures of the t and will be the same for the metal and the water.) Table 1. Specific heat capacities of various metals and other substances Specific Heat Capacity, C (J/g.°C) 0.129 0.129 0.132 0.133 Specific Heat Capacity, C (3/goC) 0.421 0.444 0.449 0.450 0.460 0.522 0.757...
Question 4 of 8 > Substance lead Specific heat capacity (J/g °C) 0.128 0.235 0.385 silver...
Question 4 of 8 > Substance lead Specific heat capacity (J/g °C) 0.128 0.235 0.385 silver copper iron 0.449 aluminum 0.903 4.184 water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 18.3 °C when 81.3 J of heat is added to the substance. What is the most likely identity of the substance? O aluminum silver O water O copper
A piece of unknown substance weighs 57.2 g and requires 3210 ) to increase its temperature...
A piece of unknown substance weighs 57.2 g and requires 3210 ) to increase its temperature from 22.6°C to 89.2°C. (a) What is the specific heat (in J/g.°C) of the substance? 493 /9-°C (6) If it is one of the substances found in the table below, what is its likely identity? Specific Heats of Common Substances at 25°C and 1 bar Substance Symbol (state) Specific Heat (1/g.c) gold Au(s) 0.129 copper Cu(s) 0.384 iron Fe(s) 0.449 argon Arg) 0.521 silicon...
6) If 15.4 g piece of aluminum is dropped into 654 g of water at 264...
6) If 15.4 g piece of aluminum is dropped into 654 g of water at 264 °C. The initial temperature of aluminum is 98.4°C. Calculate the final temperature of both water and aluminurn? (Specific heat of water and aluminum is from #1) 7) Calculate Enthalpy of the following reaction (Hz) from standard enthalpies of formation (H) from the table below. (a) C2H5OH(L) + 3 029) - 2 CO2(g) + 3 H2O(1) (b) 3 N0369) + H20(1) - 2 HNO3(aq) +...
Please answer in detail on how these 2 answers are gotten. Include Heat formula (or any...
Please answer in detail on how these 2 answers are
gotten. Include Heat formula (or any formula) and all math used to
get to answer
Calculate the mass, in grams, for each of the following using the table below Table Specific Heats of Some Substances Specific Heat (J/g C) Substance Aliminium, Al(s) Copper, Cu(s) Gold, Au(s) ron, Fe(s) Silver. Ag(s) Titanium, Ti(s) 0.897 0.385 0.129 0.452 0.235 0.523 2.04 2.46 0.864 4.184 2.03 Elements Compounds Ammonia, NHs(g) Ethanol, C2H5OHl) Sodium...
3.37 Use the heat equation to calculate the energy for each of the following (see Table...
3.37 Use the heat equation to calculate the energy for each of the following (see Table 3.11): a. calories to heat 8.5 g of water from 15 °C to 36 °C b. 2600 joules lost when 25 g of water cools from 86°C to 61 °C c. 9.3 kilocalories to heat 150 g of water from 15 °C to 77 °C d. kilojoules to heat 175 g of copper from 28 °C to 188 °C 3.38 Use the beat. cal/g...
1. A 20.0-8 piece of aluminum at 0.0°C is dropped into a beaker containing 100.0 g...
1. A 20.0-8 piece of aluminum at 0.0°C is dropped into a beaker containing 100.0 g of water. The temperature of the water drops from 90.0°C to 85.7°C. What quantity of energy did the aluminum absorb? What is the specific heat of the aluminum? 2. If 55.0 ml of water at 22.5°C is mixed with 100.0 ml of water at 95.2 'C, what would you expect for a final temperature? 3. Cold packs (the kind that get cold when you...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol)...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
Calculate the amount of heat in J required to increase the temperature of 25.0 grams of water from 25. °C to 50.0 °C. ice Specific Heats of Common Substances at 25 °C and 1 bar Substance Symbol Specific Heat (J/g (state) °C) helium He(s) 5.193 water H2O(1) 4.184 ethanol C2H60(1) 2.376 H2O(s) 2.093 (at -10 °C) water vapor H2O(g) 1.864 nitrogen N2(8) 1.040 air 1.007 oxygen O2(8) 0.918 aluminum Al(s) 0.897 carbon CO2(8) 0.853 dioxide argon Ar(s) 0.522 iron Fe(s)...
the Specific Heat Capicity of Tungsten is given here.
3. Calculate the temperature change when 32 grams of tungsten has 21 Joules of heat added to it. temperature be- in between the initial temperatures of the t and will be the same for the metal and the water.) Table 1. Specific heat capacities of various metals and other substances Specific Heat Capacity, C (J/g.°C) 0.129 0.129 0.132 0.133 Specific Heat Capacity, C (3/goC) 0.421 0.444 0.449 0.450 0.460 0.522 0.757...
Question 4 of 8 > Substance lead Specific heat capacity (J/g °C) 0.128 0.235 0.385 silver copper iron 0.449 aluminum 0.903 4.184 water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 18.3 °C when 81.3 J of heat is added to the substance. What is the most likely identity of the substance? O aluminum silver O water O copper
A piece of unknown substance weighs 57.2 g and requires 3210 ) to increase its temperature from 22.6°C to 89.2°C. (a) What is the specific heat (in J/g.°C) of the substance? 493 /9-°C (6) If it is one of the substances found in the table below, what is its likely identity? Specific Heats of Common Substances at 25°C and 1 bar Substance Symbol (state) Specific Heat (1/g.c) gold Au(s) 0.129 copper Cu(s) 0.384 iron Fe(s) 0.449 argon Arg) 0.521 silicon...
6) If 15.4 g piece of aluminum is dropped into 654 g of water at 264 °C. The initial temperature of aluminum is 98.4°C. Calculate the final temperature of both water and aluminurn? (Specific heat of water and aluminum is from #1) 7) Calculate Enthalpy of the following reaction (Hz) from standard enthalpies of formation (H) from the table below. (a) C2H5OH(L) + 3 029) - 2 CO2(g) + 3 H2O(1) (b) 3 N0369) + H20(1) - 2 HNO3(aq) +...
Please answer in detail on how these 2 answers are
gotten. Include Heat formula (or any formula) and all math used to
get to answer
Calculate the mass, in grams, for each of the following using the table below Table Specific Heats of Some Substances Specific Heat (J/g C) Substance Aliminium, Al(s) Copper, Cu(s) Gold, Au(s) ron, Fe(s) Silver. Ag(s) Titanium, Ti(s) 0.897 0.385 0.129 0.452 0.235 0.523 2.04 2.46 0.864 4.184 2.03 Elements Compounds Ammonia, NHs(g) Ethanol, C2H5OHl) Sodium...
3.37 Use the heat equation to calculate the energy for each of the following (see Table 3.11): a. calories to heat 8.5 g of water from 15 °C to 36 °C b. 2600 joules lost when 25 g of water cools from 86°C to 61 °C c. 9.3 kilocalories to heat 150 g of water from 15 °C to 77 °C d. kilojoules to heat 175 g of copper from 28 °C to 188 °C 3.38 Use the beat. cal/g...
1. A 20.0-8 piece of aluminum at 0.0°C is dropped into a beaker containing 100.0 g of water. The temperature of the water drops from 90.0°C to 85.7°C. What quantity of energy did the aluminum absorb? What is the specific heat of the aluminum? 2. If 55.0 ml of water at 22.5°C is mixed with 100.0 ml of water at 95.2 'C, what would you expect for a final temperature? 3. Cold packs (the kind that get cold when you...
Substance molar heat capacity (C.)/J•mol-1.°C-1 75.3 specific heat capacity (C.) /J•g-lo°C-1 0.384 H2O(1) Cu(s) C,H,OH(l) (ethanol) Fe(s) 111.5 0.449 1. Fill in the empty entries in the table above. 2. If the same amount of energy is transferred to 1.0 g samples of each of the substances listed above, order them from largest AT to smallest AT. Explain. 3. Which is the consequence of copper's relatively low specific heat (0.385 J/(g°C)) compared to water (4.18 J/(g°C)) on the temperature change...
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