A list of the calorie content of foods indicates that a cup of frozen strawberries contains 224 Calories. Express this value in kJ and in J. 9.37E-1 kJ 937 J 1 cal = 4.184 J
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- Consider the problem below: (Equation 1) 4 CO(g) + 4 H2O(l) ---> C4H8(l) + 4 O2(g) ΔH = 890.6 kJ/mol (Equation 2) CO2(g) ---> CO(g) + 1/2 O2(g) ΔH = 90.6 kJ/mol (Equation 3) C4H8(l) + 6 O2(g) ---> 4 CO2(g) + 4 H2O(l) ΔH = ??????? The ΔH for equation 3 is:______(express in kJ) Screen Reader Version Consider the problem below: (Equation 1) 4 CO(g) + 4 H2O(l) arrow C4H8(l) + 4 O2(g) ΔH = 890.6 kJ/mol (Equation 2) CO2(g) arrow C O(g) + 1/2 O2(g) ΔH = 90.6 kJ/mol (Equation 3) C4H8(l) + 6 O2(g) arrow 4 CO2(g) + 4 H2O(l) ΔH = ??????? The ΔH for equation 3 is:______(express in kJ)Calculate the heat reaction in Mg given: Mass of Mg: 1.07786g Volume HCl: 50mL of 3M HCl Heat capacity of the solution: 4.184J/gx°C Trial 1 initial temperature: 26°C Trial 1 final temperature: 47°C Trial 2 Initial Temperature: 27°C Trial 2 final temperature: 47°C Note: please give detailed solutions. Thank you!Calculate Ksp for the salt NaCl at 25°C. Substance ΔGf°(in kJ/mol) Na+(aq) –262.0 Cl–(aq) –131.0 NaCl(s) -383.6
- Calculate Q (system) (J) and delta H (kJ/mol). Use data below and from methods: Mass of NaNO3 required (already calculated) = 8.5 grams Initial Temperature ti (0C) = 25.0 0C Temperature after 240 sectons (tf, final temp) = 19.0 0C Measuring the heat evolved or absorbed methods Weigh the calculated mass of NaNO3 needed to prepare 100mL of a 1.0M solution. Place 100mL of distilled water in the calorimeter and carefully add the solid NaNO3. Begin stirring and measure the temperature of the solution to the nearest 0.10C after 30seconds and every 30 seconds thereafter until the temperature attains either a maximum or minimum which is the final temperature tf. Calculate q(system), using specific heat=4.184J/g.0C, density ofsolution=1.0g/mL; heat capacity of calorimeter = 10J/0C Calculate the enthalpy change DH from q(system) and the number of moles NaNO3Cp is greater than or equal to Cv. Why?my approach was using q = I∆φ∆t and i got 1980J, converted it to kj -> q=1.98kj. using ∆U = qV , ∆U =1.98kj. is my attempt correct???
- The specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?Given the standard molar enthalpy of formation of hexane is -167.2 kj/mol, determine the C-C bond dissociation energy of cyclohexane.need energy for BDE(C-C) and its standard deviationunit kJ/molA sample of methylhydrazine (rocket fuel) weighing 1.500 g was ignited in a bomb calorimeter initially at 25.0°C, producing a temperature rise of 10.215 K. Determine the internal energy (∆U) of combustion of methylhydrazine. a) To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.5000 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K. b) Using the calorimeter constant, determine ∆U, in kJ/mol, of combustion of the methylhydrazine (CH₆N₂, MW 46.10 g/mol).
- qsystem = -1834.3J, with a mZn = 34.8g (cZn = 0.390J/goC), What is the ∆T given the heat loss?A sample of methylhydrazine (rocket fuel) weighing 1.500 g was ignited in a bomb calorimeter initially at 25.0°C, producing a temperature rise of 10.215 K. Determine the internal energy (∆U) of combustion of methylhydrazine. To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.6500 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K.To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.4500 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K.