1.
The heat capacity of a calorimeter is given as 1264 J/oC. Suppose the enthalpy of solution for calcium chloride (MM=111 g/mol) in water is given by the thermochemical equation:
CaCl2(s) + H2O(l) → Ca2+(aq) + 2Cl-(aq) ΔH = -81.0 kJ/mol.
Calculate the temperature change if 11.1 g of calcium chloride is dissolved in water in the calorimeter.
2.
Given the following data, calculate ΔH for the reaction of two moles of carbon monoxide with oxygen gasto give carbon dioxide.
2 C (s) + O2 (g) → 2 CO (g) ΔH = -221.0 kJ
3.
The heat capacity of a calorimeter is given as 1264 J/oC. Suppose the enthalpy of solution for calcium chloride (MM=111 g/mol) in water is given by the thermochemical equation:
CaCl2(s) + H2O(l) → Ca2+(aq) + 2Cl-(aq) ΔH = -81.0 kJ/mol.
Calculate the temperature change if 11.1 g of calcium chloride is dissolved in water in the calorimeter.
C (s) + O2 (g) → CO2 (g) ΔH = - 393.5 kJ
1. The heat capacity of a calorimeter is given as 1264 J/oC. Suppose the enthalpy of...
When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0 C to 38.7 C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 0.710 mol of calcium chloride dissolves in water? The solution process is CaCl2(s) --> Ca2+(aq) + 2Cl–(aq)
please answer for a thumbs up! 1. Given the standard enthalpy changes for the following two reactions: (1) Ni(s) + Cl2(g)--->NiCl2(s)...... ΔH° = -305.3 kJ (2) Fe(s) + Cl2(g)-->FeCl2(s)......ΔH° = -341.8 kJ what is the standard enthalpy change for the reaction: (3) Ni(s) + FeCl2(s)--->NiCl2(s) + Fe(s)......ΔH° = ? ____ kJ 2- When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory...
1. How much heat is needed to raise the temperature of 1.50 g of aluminum metal from 23.2 °C to 30.5 °C? (Specific heat capacity of aluminum is 0.90 J/g-K). 2. Given the following thermochemical equation: DH = -1107 kJ How many kJ of heat are released when 15.75 g of Ba(s) reacts completely with oxygen to form BaO(s)? 3. Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.25 g naphthalene is burned in a bomb calorimeter, the temperature rises from 25.25...
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter In the laboratory a general chemistry student finds that when 1.85 g of CaCl2(s) are dissolved in 114.50 g of water, the temperature of the solution increases from 23.01 to 25.89 °C The heat capacity of the calorimeter (sometimes referred to as the calortmeter constant) was determined in a separate experiment to be 1.71 J/OC...
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
Heat Capacity and Calorimetry A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25C to 33.73C. If the heat capacity of the calorimeter and contents is 9.63kJ/C, what is the value of q for burning 1.00 lol of ethanol at constant volume and 25.00C. Is q equal to U or H? 214e Questions and Problems the enthalpy change when 0.710 mol of calcium...
Consider the dissolution of Calcium Chloride: CaCl2(s)---->Ca^+2(aq) + 2Cl−(aq) ΔHrxn= -81.5kJ An 12.0 g sample of calcium chloride is dissolved in 100.0 g of water, with both substance at 22.0 degree C. Molar Mass: CaCl2= 110.98g.mol Molar Mass H20= 18.02g/mol Density of H20= 1.00g/mol Cs(soln)= 4.20 J/(g K) Will the temperature of the solution go up or down? Explain. Calculate q(reaction)
An 78.5 g piece of metal whose T = 63.00 oC is placed in a coffee cup calorimeter containing 125 g water. When the system reaches equilibrium, the water has changed from 20.00 oC to 24.00 oC. What is specific heat of metal? An 88.5 g piece of metal whose T = 78.8 oC is placed in a coffee cup calorimeter containing 244 g water. When the system reaches equilibrium, the water has changed from 18.80 oC to 200 oC....
a) Use Hess's law to calculate the enthalpy change for the reaction: 3C(s) + 4H2(g) + ½O2(g) → C3H8O(l) Given the following thermochemical equations: 2C3H8O(l) + 9O2(g) → 6CO2(g) + 8H2O(l) ΔH = -4042.6 kJ/mol C(s) + O2(g) → CO2(g) ΔH = -393.51 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔH = -285.83 kJ/mol (in kJ/mol) A: -267.7 B: -302.6 C: -341.9 D: -386.3 E: -436.5 F: -493.3 G: -557.4 H: -629.9 b) Define if the following statement is an endothermic process or exothermic...