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1. How much heat is required at constant pressure to melt 1 mole of ice at...
82. Calculate A Hex for the reaction. CH4(8) + 4 C12(8) — CCl4(8) + 4 HCl(8)...
82. Calculate A Hex for the reaction. CH4(8) + 4 C12(8) — CCl4(8) + 4 HCl(8) Use the following reactions and given AH's: C(s) + 2 H2(8) — CH4(8) AH = - 74.6 kJ. C(s) + 2 C12(8) - CĊ14(8) AH = -95.7 kJ X2 H2(8) + Cl2(8) —> 2HCl(8) AH = -92.3 kJ_x2 x 2 X2
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations:...
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations: C(s)+H2(g)-->CH4 H= -74.6 kJ C(s) + Cl2(g)--> CCl4 H=-95.7 kJ H2(g)+Cl2(g)--> HCl H=-92.3 kJ
Gen Chem I Fa17 York, Exam 2 Show all work, include units as appropriate 1. Use...
Gen Chem I Fa17 York, Exam 2 Show all work, include units as appropriate 1. Use the given standard enthalpies of formation to calculate AH° for the following reaction: CH4(9) + 4C4;() --> CC14(g) + 4HCl(3) Species AH', kJ/mol CH4(g) -74.6 Cl2(g) CCL(3) -95.7 HCl(9) -92.3 0
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to...
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to steam at 100 C?Specific heat of ice: 2.09 J/g * C DHfus = 6.02 kJ/molSpecific heat of water: 4.18 J/g * C DHvap = 40.7 kJ/molSpecific heat of steam: 1.84 J/g * C
You have a 1.08-mole sample of water at -33°C, and you heat it until you have...
You have a 1.08-mole sample of water at -33°C, and you heat it until you have gaseous water at 135°C. Calculate q for the entire process. Use the following data. Specific heat capacity of ice = 2.08 ) •c-1-1 Specific heat capacity of water = 4.18 •c-1g-1 Specific heat capacity of steam = 2.02 ºc-1 9-1 H20(s) → H20(1) H20(1)→ H20(9) AH fusion = 6.01 kJ/mol (at 0°C) AH vaporization = 40.7 kJ/mol (at 100°C) k] Need Help? Read It...
if u can show how u do each one, that would be amazing! How much heat...
if u can show how u do each one, that would be
amazing!
How much heat is required to convert 90 g of ice at - 40.0°C into water at 60.0°C? The specific heats (Cs) of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H0 AH A) 60.1 kJ = 6.01 kJ/mol, and AH B) 18.8 kJ -40.67 kJ/mol. C) 45.1 kJ D) 37.6 kJ E) 30.5 kJ 11. What is correct for a...
11. The following would be required for calculations of heat flow in which of the heating...
11. The following would be required for calculations of heat flow in which of the heating curve steps ? Molar heat of vaporization of water (AH vap = 40.7 kJ/mol) Specific heat of ice (Cice = 2.09 J/g °C) Molar heat of fusion of water (AH fus = 6.02 kJ/mol) Specific heat of water (C H20 = 4.18 J/g °C) Specific heat of steam(C steam = 2.01 J/g °C) Heating Curve for Water Degrees Celsius -50+ 0 400 800 1200...
calculate the molar heat capacity Cm for water. you knew that 30.1 kJ was required to...
calculate the molar heat capacity Cm for water. you knew that 30.1 kJ was required to heat 10.0 g of ice from 0.00 C to steam 100.00 C and that the melting point pin ∆fusH = 6.01 kJ / mol and the evaporating enthalpy ∆vapH = 40.7 kJ / mol.
How much heat is required to warm to 0 degrees C and then melt a 100ml...
How much heat is required to warm to 0 degrees C and then melt a 100ml block of ice( at 20 degrees C) that is 100ml in volume? Density of ice is 0.92 g/ml. DeltaHfus=6.01 kJ/mol. DeltaHvap=44kj/mol. Heat capacity of ice= 2.09 j/g C. Heat capacity of water= 4.184 J/g C.
How many grams of steam at 100C are required to melt 200 grams of ice? Heat...
How many grams of steam at 100C are required to melt 200 grams of ice? Heat fusion for ice at 0C is 334J/g. Heat of vaporization of water at 100C is 2,230J/g.
82. Calculate A Hex for the reaction. CH4(8) + 4 C12(8) — CCl4(8) + 4 HCl(8) Use the following reactions and given AH's: C(s) + 2 H2(8) — CH4(8) AH = - 74.6 kJ. C(s) + 2 C12(8) - CĊ14(8) AH = -95.7 kJ X2 H2(8) + Cl2(8) —> 2HCl(8) AH = -92.3 kJ_x2 x 2 X2
Gen Chem I Fa17 York, Exam 2 Show all work, include units as appropriate 1. Use the given standard enthalpies of formation to calculate AH° for the following reaction: CH4(9) + 4C4;() --> CC14(g) + 4HCl(3) Species AH', kJ/mol CH4(g) -74.6 Cl2(g) CCL(3) -95.7 HCl(9) -92.3 0
You have a 1.08-mole sample of water at -33°C, and you heat it until you have gaseous water at 135°C. Calculate q for the entire process. Use the following data. Specific heat capacity of ice = 2.08 ) •c-1-1 Specific heat capacity of water = 4.18 •c-1g-1 Specific heat capacity of steam = 2.02 ºc-1 9-1 H20(s) → H20(1) H20(1)→ H20(9) AH fusion = 6.01 kJ/mol (at 0°C) AH vaporization = 40.7 kJ/mol (at 100°C) k] Need Help? Read It...
if u can show how u do each one, that would be
amazing!
How much heat is required to convert 90 g of ice at - 40.0°C into water at 60.0°C? The specific heats (Cs) of ice, water, and steam are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK, respectively. For H0 AH A) 60.1 kJ = 6.01 kJ/mol, and AH B) 18.8 kJ -40.67 kJ/mol. C) 45.1 kJ D) 37.6 kJ E) 30.5 kJ 11. What is correct for a...
11. The following would be required for calculations of heat flow in which of the heating curve steps ? Molar heat of vaporization of water (AH vap = 40.7 kJ/mol) Specific heat of ice (Cice = 2.09 J/g °C) Molar heat of fusion of water (AH fus = 6.02 kJ/mol) Specific heat of water (C H20 = 4.18 J/g °C) Specific heat of steam(C steam = 2.01 J/g °C) Heating Curve for Water Degrees Celsius -50+ 0 400 800 1200...
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