Calculate the entropy change from burning 67.3 g of solid glucose (C6H12O6, molar mass 180.2 g/mol) to produce gaseous carbon dioxide and gaseous water, using the values in the table below.
Substance | S0 / J K-1 mol-1 |
Glucose(s) | 209.2 |
O2(g) | 205.15 |
CO2(g) | 213.79 |
H2O(g) | 188.84 |
Calculate the entropy change from burning 67.3 g of solid glucose (C6H12O6, molar mass 180.2 g/mol)...
Calculate the entropy change from burning 41.1 g of solid glucose (C6H1206, molar mass 180.2 g/mol) to produce gaseous carbon dioxide and gaseous water, using the values in the table below. S0/JK mor Substance Glucose(s) O2(g) CO2(g) H2O(g) 209.2 205.15 213.79 188.84 Select one: a. 4.01e4 J/K b. 223 J/K C. -2.67 J/K d. None of the other options e. -482 J/K
Calculate the entropy change from burning 41.1 g of solid glucose (C6H1206, molar mass 180.2 g/mol) to produce gaseous carbon dioxide and gaseous water, using the values in the table below. Substance º/JK' mort Glucose(s) 209.2 02(9) 205.15 CO2(g) 213.79 H2009) 188.84 Select one: a. 4.01e4 J/K o b. 223 JIK O C.-2.67 J/K d. None of the other options. e-482 J/K
Calculate the molality of a glucose solution, C6H12O6 (molar mass=180.2 g/mol) that is prepared by mixing 234 g of glucose in 755 g water
Answer the following questions about the fermentation of glucose (C6H12O6 , molar mass 180.2 g/mol) to ethanol (C2H6O) and CO2. C6H12O6(s) → 2 C2H6O(l) + 2 CO2(g) Δ H = −16 kcal/mol glucose ethanol How many kilocalories of energy are released from 54.0 g of glucose?
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol ______kJ/mol
Calculate the standard enthalpy change for the fermentation process, in which glucose (C6H12O6) is converted into ethanol (C2H5OH) and carbon dioxide (CO2). Substance Enthalpy of Formation, Δ H o f CO2 (g) −393.5 kJ/mol CO2 (aq) −412.9 kJ/mol C2H5OH (l) −276.98 kJ/mol C6H12O6 (s) −1,274.5 kJ/mol H2O (g) −241.8 kJ/mol H2O (l) −285.8 kJ/mol O2 (g) 0 kJ/mol
1) if 6.85 of glucose( C6H12O6, molar mass=180.2 g/mol) is dissolved in 155g of chloroform( CHCL3,molar mass= 119.4 g/mol) , what is the boiling point of the solution. ( the boiling point of pure CHCl3 is 61.2 celsius, and Kb = 3.63 celsius/m for CHCl3) 2) a,) Liquid ammonia (boiling point = -33.4C) can be used as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(l) from -65.0C to -12.0C? Heat of...
please help with this If 1.15 g of glucose (molar mass = 180.2 g/mol) is burned in a calorimeter, the temperature increases from 23.40 degrees Celsius to 27.21 degrees Celsius. if the heat capacity of the calorimeter is 958 J/ degrees celsius and the calorimeter contains 899.5 g of water, calculate the amount of heat given off per mole of glucose under these conditions.
The human body converts glucose (C6H12O6) to carbon dioxide and water. The balanced chemical equation for the reaction is: C6H12O6 + 6 O2 → 6 CO2 + 6 H2O If you ate a candy bar that contained 22.2 g of glucose (C6H12O6), how many grams of water will the body produce from the glucose you ate? How many grams of CO2 would that make?
Calculate the standard-state entropy for the following reaction: 6 CO2(g) + 6 H2O(l) ⟶ 1 C6H12O6(s) + 6 O2(g) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) C6H12O6(s) 212 O2(g) 205 CO2(g) 214 H2O(l) 189