16.41 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by...
16.41 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.7°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
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16.41 g of MgSO₄ is placed into 100.0 mL of water. The water's
temperature increases by...
Question 29 of 50 Submit 5.21 g of MgSO4 is placed into 100.0 mL of water....
Question 29 of 50 Submit 5.21 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4 (The spe- cific heat of water is 4.18 J/g. *C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. kJ/mol 1 2 3 C +/- : 0 x 100
Using the equations Ca (s)2 O (g) Сао (s) 2 H2 (g) Determine the enthalpy for...
Using the equations Ca (s)2 O (g) Сао (s) 2 H2 (g) Determine the enthalpy for the reaction Са (s) + 2 H0 () — Са(ОН)2 (s) + H2 (9). CaO (s) AH° = -635 kJ/mol -64 kJ/mol H2O ()Ca(OH)2 (s) AH O2 (g)2 H2O (I) AH° = -572 kJ/mol kJ/mol 1 2 3 4 6 C 5 7 8 9 +/- 0 x 100 LO 11.01 g of MgSO4 is placed into 100.0 mL of water. The water's temperature...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of...
A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.0°C and the temperature of the resulting solution was recorded as 37.0°C, determine the DH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2)that the density(1.00 g/mL) and the specific...
0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution....
0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 8.41°С. Calculate AH for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g•°C and the density of the solution is 1.02 g/mL). | kJ/mol
Question 44 of 50 Submit 3.15 mol of an unknown solid is placed into enough water...
Question 44 of 50 Submit 3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 19.21°C. Calculate AH for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g.°C and the density of the solution is 1.20 g/mL). kJ/mol 1 2 3 C +/- : 0 x 100
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee- cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. - 131 kJ O -613 kJ O-328 kJ 0 -28.3 kJ
What is the final temperature of the solution when 4.806 g of sodium hydroxide is dissolved in 100.0 mL of water at an i...
What is the final temperature of the solution when 4.806 g of sodium hydroxide is dissolved in 100.0 mL of water at an initial temperature of 24.5 C?. The density of water is 0.9969 g/cm3, and the heat capacity is 4.184 J/C. The enthalpy of dissolution for sodium hydroxide is -44.2 kJ/mol.
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water...
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water in a coffee cup calorimeter. The water was initially at 20.0°C and the final temperature of the resulting solution was recorded as 17.1°C. Calculate the experimental AHcoln (in units of kJ/mol NH.NO:) for the dissolution of NH NO3 (molar mass = 80.04 g/mol). Assume that no heat is lost to the calorimeter or the surroundings. The density of water is 1.00 g/mL and the...
4. 100.0 mL of water is placed in a calorimeter and allowed to reach an initial...
4. 100.0 mL of water is placed in a calorimeter and allowed to reach an initial temperature of 23°C. A 45.0g block of Cu (SH=0.385 J/g at 285°C is placed in the water (SH = 4.18 J/g. C) in the calorimeter. a) If the final temperature reached is 30°C, determine the heat capacity of the calorimeter? b) The same calorimeter was used to determine the heat of solution of 20.0g of NH4NO3 NH4NO3 (s) + NH4NO3 (29) The initial temperature...
specific heat capacity 2. If 3.8 g of calcium chloride (CaCl2) is dissolved in 100.0 mL...
specific heat capacity
2. If 3.8 g of calcium chloride (CaCl2) is dissolved in 100.0 mL of water, the following data are collected: starting temperature is 25.8 °C, final temperature after dissolving is 29.9 °C. Calculate the enthalpy of solution in Joules. You may assume a density of 1.00 g/mL for the solution and you may assume that the specific heat is that of water (this is a dilute solution) and is 4.18 J/(gx°C). Is this an endothermic or exothermic...
Question 29 of 50 Submit 5.21 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4 (The spe- cific heat of water is 4.18 J/g. *C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. kJ/mol 1 2 3 C +/- : 0 x 100
Using the equations Ca (s)2 O (g) Сао (s) 2 H2 (g) Determine the enthalpy for the reaction Са (s) + 2 H0 () — Са(ОН)2 (s) + H2 (9). CaO (s) AH° = -635 kJ/mol -64 kJ/mol H2O ()Ca(OH)2 (s) AH O2 (g)2 H2O (I) AH° = -572 kJ/mol kJ/mol 1 2 3 4 6 C 5 7 8 9 +/- 0 x 100 LO 11.01 g of MgSO4 is placed into 100.0 mL of water. The water's temperature...
0.700 moles of an unknown solid is placed into water to make 150.0 mL of solution. The solution's temperature decreases by 8.41°С. Calculate AH for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g•°C and the density of the solution is 1.02 g/mL). | kJ/mol
Question 44 of 50 Submit 3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 19.21°C. Calculate AH for the dissolution of the unknown solid. (The specific heat of the solution is 4.18 J/g.°C and the density of the solution is 1.20 g/mL). kJ/mol 1 2 3 C +/- : 0 x 100
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee- cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. - 131 kJ O -613 kJ O-328 kJ 0 -28.3 kJ
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water in a coffee cup calorimeter. The water was initially at 20.0°C and the final temperature of the resulting solution was recorded as 17.1°C. Calculate the experimental AHcoln (in units of kJ/mol NH.NO:) for the dissolution of NH NO3 (molar mass = 80.04 g/mol). Assume that no heat is lost to the calorimeter or the surroundings. The density of water is 1.00 g/mL and the...
4. 100.0 mL of water is placed in a calorimeter and allowed to reach an initial temperature of 23°C. A 45.0g block of Cu (SH=0.385 J/g at 285°C is placed in the water (SH = 4.18 J/g. C) in the calorimeter. a) If the final temperature reached is 30°C, determine the heat capacity of the calorimeter? b) The same calorimeter was used to determine the heat of solution of 20.0g of NH4NO3 NH4NO3 (s) + NH4NO3 (29) The initial temperature...
specific heat capacity
2. If 3.8 g of calcium chloride (CaCl2) is dissolved in 100.0 mL of water, the following data are collected: starting temperature is 25.8 °C, final temperature after dissolving is 29.9 °C. Calculate the enthalpy of solution in Joules. You may assume a density of 1.00 g/mL for the solution and you may assume that the specific heat is that of water (this is a dilute solution) and is 4.18 J/(gx°C). Is this an endothermic or exothermic...
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