Be sure to answer all parts. A 0.4875−g sample of solid magnesium is burned in a...
Be sure to answer all parts. A 0.4875−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 3.991°C. (a) Calculate the heat given off by the burning Mg in kJ/g. kJ/g (b) Calculate the heat given off by the burning Mg in kJ/mol. kJ/mol
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Be sure to answer all parts. A 0.4875−g sample of solid
magnesium is burned in a...
Be sure to answer all parts. A 0.4275 g sample of solid magnesium is burned in...
Be sure to answer all parts. A 0.4275 g sample of solid magnesium is burned in a constant volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 3.499°C. (a) Calculate the heat associated with the burning Mg in kJ/g. kJ/g (b) Calculate the heat associated with the burning of Mg in kJ/mol. kJ/mol
A 0.2075−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a...
A 0.2075−g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 1.700°C. (a) Calculate the heat given off by the burning Mg in kJ/g. kJ/g (b) Calculate the heat given off by the burning Mg in kJ/mol. kJ/mol
4 10empts let Check my work Be sure to answer all parts. A0.4775 g sample of...
4 10empts let Check my work Be sure to answer all parts. A0.4775 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has m heat capacity of 3024 JeC. The temperature increases by 3.909°C. ts (a) Calculate the heat associated with the burning Mg in kJ/g kJ/g eBook (b) Calculate the heat associated with the burning of Mg in kJ/mol Pont kJ/mol eferences rew <Erex D Type here to search
will you please help me with 7 and 8? 18 15 = 7. A 0.1036 g...
will you please help me with 7 and 8?
18 15 = 7. A 0.1036 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/ °C. The calorimeter contains exactly 200 g of water, and the temperature increases by 0.913 °C. Calculate the heat given off by the burning Mg in kJ/mol. BOX OOD FS 1620 8. Calculate the heat of combustion for the following reaction from the standard enthalpies...
A 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat...
A 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/C. If the temperature rise of the calorimeter with water was 1.25*C, calculate the enthalpy of combustion(in kJ/mol) of magnesium. Mg(s) + 1/2O2(g) -> MgO(s) Write answer to three significant figures. Numeric Response
HQ11.30 Homework Answered When 0.1625 g of magnesium is burned in a bomb calorimeter that has...
HQ11.30 Homework Answered When 0.1625 g of magnesium is burned in a bomb calorimeter that has a heat capacity of 3.03 kJ/°C, the temperature increases by 1.252°C. How much heat (kJ/mol) is liberated during the burning of the magnesium? Numeric Answer:
A 1.87 g sample of lauric acid (C12H2402), a common constituent of fats, is burned in...
A 1.87 g sample of lauric acid (C12H2402), a common constituent of fats, is burned in a bomb calorimeter. The temperature of the calorimeter increases by 47.8°C (Celsius). Given that the energy of combustion (AE) for lauric is -37.1 kJ/g, calculate the heat capacity of the bomb calorimeter. Make sure you enter kJ/C for your unit behind the number. heat capacity of the calorimeter =
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess...
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify...
A 0.559-g sample of 9,10-anthracenedione (C14H302) is burned in a bomb calorimeter and the temperature increases...
A 0.559-g sample of 9,10-anthracenedione (C14H302) is burned in a bomb calorimeter and the temperature increases from 24.50 °C to 27.50 °C The calorimeter contains 1.15x10g of water and the bomb has a heat capacity of 876J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 9,10-anthracenedione burned (kJ/mol). C14H2O2() + 15 O2(g)— 14 CO2(g) + 4H2O(1) E k J/mol
A 0.375-g sample of 2-naphthylacetic acid (C12H1002) is burned in a bomb calorimeter and the temperature increases from...
A 0.375-g sample of 2-naphthylacetic acid (C12H1002) is burned in a bomb calorimeter and the temperature increases from 25.80 °C to 28.00 °C. The calorimeter contains 1.06x103 g of water and the bomb has a heat capacity of 903 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 2-naphthylacetic acid burned (kJ/mol). C12H1002()+27/2 O2(g) —>12 CO2(g) +5 H2O(1) AE = kJ/mol
Be sure to answer all parts. A 0.4275 g sample of solid magnesium is burned in a constant volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 3.499°C. (a) Calculate the heat associated with the burning Mg in kJ/g. kJ/g (b) Calculate the heat associated with the burning of Mg in kJ/mol. kJ/mol
4 10empts let Check my work Be sure to answer all parts. A0.4775 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has m heat capacity of 3024 JeC. The temperature increases by 3.909°C. ts (a) Calculate the heat associated with the burning Mg in kJ/g kJ/g eBook (b) Calculate the heat associated with the burning of Mg in kJ/mol Pont kJ/mol eferences rew <Erex D Type here to search
will you please help me with 7 and 8?
18 15 = 7. A 0.1036 g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/ °C. The calorimeter contains exactly 200 g of water, and the temperature increases by 0.913 °C. Calculate the heat given off by the burning Mg in kJ/mol. BOX OOD FS 1620 8. Calculate the heat of combustion for the following reaction from the standard enthalpies...
A 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/C. If the temperature rise of the calorimeter with water was 1.25*C, calculate the enthalpy of combustion(in kJ/mol) of magnesium. Mg(s) + 1/2O2(g) -> MgO(s) Write answer to three significant figures. Numeric Response
HQ11.30 Homework Answered When 0.1625 g of magnesium is burned in a bomb calorimeter that has a heat capacity of 3.03 kJ/°C, the temperature increases by 1.252°C. How much heat (kJ/mol) is liberated during the burning of the magnesium? Numeric Answer:
A 1.87 g sample of lauric acid (C12H2402), a common constituent of fats, is burned in a bomb calorimeter. The temperature of the calorimeter increases by 47.8°C (Celsius). Given that the energy of combustion (AE) for lauric is -37.1 kJ/g, calculate the heat capacity of the bomb calorimeter. Make sure you enter kJ/C for your unit behind the number. heat capacity of the calorimeter =
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify...
A 0.559-g sample of 9,10-anthracenedione (C14H302) is burned in a bomb calorimeter and the temperature increases from 24.50 °C to 27.50 °C The calorimeter contains 1.15x10g of water and the bomb has a heat capacity of 876J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 9,10-anthracenedione burned (kJ/mol). C14H2O2() + 15 O2(g)— 14 CO2(g) + 4H2O(1) E k J/mol
A 0.375-g sample of 2-naphthylacetic acid (C12H1002) is burned in a bomb calorimeter and the temperature increases from 25.80 °C to 28.00 °C. The calorimeter contains 1.06x103 g of water and the bomb has a heat capacity of 903 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of 2-naphthylacetic acid burned (kJ/mol). C12H1002()+27/2 O2(g) —>12 CO2(g) +5 H2O(1) AE = kJ/mol
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