A 0.0593−mol sample of a nutrient substance, with a formula
weight of 114 g/mol, is burned in a bomb calorimeter containing
4.73 × 102 g H2O. Given that the fuel value
is 4.80 ×10−1 in nutritional Cal when the temperature of
the water is increased by 6.86°C, calculate the fuel value in
kJ.
Enter your answer in scientific notation. Be sure to answer all
parts.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
A 0.0593−mol sample of a nutrient substance, with a formula weight of 114 g/mol, is burned...
A 4.11−g sample of octane is burned in a bomb calorimeter containing 2.00 × 102 g H2O. How much energy, in cal, is released if the water temperature increases 5.33°C? Express your answer in scientific notation. Enter your answer in the provided box.
A 5.03 g sample of octane is burned in a bomb calorimeter containing 2.00 x 102 g H2O. How much energy, in cal, is released if the water temperature increases 7.52 °C? Express your answer in scientific notation. Enter your answer in the provided box. x 10 (select) cal
A 4.03−g sample of octane is burned in a bomb calorimeter containing 2.00 × 10^2 g H2O. How much energy, in cal, is released if the water temperature increases 4.58°C? Express your answer in scientific notation. Enter your answer in the provided box.
A 8.82 g sample of octane is burned in a bomb calorimeter containing 2.91 x 102 g H20. Given that 1.29 x 103 cal of energy is released if the water temperature increases 4.42°C. Calculate the energy released in J. Enter your answer in scientific notation. Be sure to answer all parts. x 10 (selec) ,
A 0.44 mol sample of a substance is burned in a bomb calorimeter with a heat capacity of 8.87 kJ/C. The temperature increases by 8.36 C. What is ΔHrxn (in kJ/mol) for the combustion of the substance?
QUESTION 17 Calculate the heat evolved by the reaction of 45.7 g of a substance burned in a bomb calorimeter knowing that the temperature of the water in the calorimeter increased by 3.90°C and the calorimeter constant is Ccal - 39.97 kJ/°C. OA -1.559x102 kJ OB. 1.559x102k1 Oc 1.559 kJ Op 1.559
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C, what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol. C2H5OH(l) + O2(g) → CO2(g) + H2O(g) ΔH°rxn = ? (Points : 1) -1.24 × 103 kJ/mol +1.24 × 103 kJ/mol -8.09 × 103 kJ/mol -9.55 × 103 kJ/mol...
A 17.5g sample of a candy bar is burned in a bomb calorimeter. which has a heat capacity of 8.75 kJ/degrees C. The temperature increases from 20.2 degrees C to 59.9 degrees C 03 Question (5 points) See page 413 A 17.5 g sample of a candy bar is burned in a bomb calorimeter, which has a heat capacity of 8.75 kJ/°C. The temperature increases from 20.2°C to 59.9°C. 1st attempt Part 1 (2.5 pts) M See Periodic Table O...
A 0.456 g (176.1 g/mol) sample of acid in question 11 is burned in a bomb calorimeter. Calculate the change in enthalpy if the temperature for 1350 g of water in the calorimeter changes from 21.5 oC to 30.4 oC. The heat capacity of the calorimeter is 564 kJ/oC.