work is done by the reaction and thus it is positive i.e, W = + 1.7* 103 J
Heat energy is absorbed by the reaction thus it is positive i.e, Q = 30.6 * 103 J
Change in internal energy = Q + W, = 1.7* 103 J + 30.6 * 103 J ; = 32.3 KJ
5. (4 points) When a particular reaction is run at a constant pressure, 1.7 kJ of...
At constant volume, the heat of combustion of a particular compound is -3952.0 kJ/mol. When 1.211 g of this compound (molar mass = 130.08 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 4.453 ◦C. What is the heat capacity (calorimeter constant) of the calorimeter?-qrxn = qcalorimeterWhat is the formula for heat (q) for the calorimeter?___________________Did the calorimeter absorb/release heat? Circle your answer.Calculate the energy absorbed by the calorimeter.Solve:
An ideal gaseous reaction occurs at a constant pressure of 35.0 atm and releases 55.8 kJ of heat. Before the reaction, the volume of the system was 8.20 L. After the reaction, the volume of the system was 3.01 L. Calculate the total change in internal energy for the system.
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following figure. When the gas undergoes a particular chemical reaction, it absorbs 822 J of heat from its surroundings and has 0.69 kJ of P−V work done on it by its surroundings. What is the value of ΔH for this process? Express your answer with the appropriate units.
A gas is confined to a cylinder under constant atmospheric pressure, as illustrated in the following figure. When the gas undergoes a particular chemical reaction, it absorbs 822 J of heat from its surroundings and has 0.69 kJ of P−V work done on it by its surroundings. What is the value of ΔE for this process? Express your answer with the appropriate units.
A 1.40-mol sample of hydrogen gas is heated at constant pressure from 304 K to 426 K. (a) Calculate the energy transferred to the gas by heat. kJ (b) Calculate the increase in its internal energy. kJ (c) Calculate the work done on the gas. kJ
A 1.90-mol sample of hydrogen gas is heated at constant pressure from 306 K to 416 K. (a) Calculate the energy transferred to the gas by heat. kJ (b) Calculate the increase in its internal energy. kJ (c) Calculate the work done on the gas. kJ
1. If q 60 kJ and w = 96 kJ for a certain process, that process (3) a. requires a catalyst. b. is endothermic. c. occurs slowly. d. is exothermic. e. cannot occur. 2. What is the change in internal energy of the system (AU) if 71 kJ of heat energy is absorbed by the system and 12 kJ of work is done on the system for a certain process? (4) a. 83 kJ b. 59 kJ c. 71 kJ...
SerCP10 12.P.003.MI.FB -/6.25 points 1 Gas in a container is at a pressure of 1.7 atm and a volume of 3.0 m3. (a) what is the work done on the gas if it expands at constant pressure to twice its initial volume? (b) What is the work done on the gas if it is compressed at constant pressure to one-quarter of its initial volume? Need Help? Read It Master It SerCP10 12.P.009.WI 3. -/6.25 points One mole of an ideal...
Calculate the w, (in kJ) when gas expards from 15L to you against a constant external pressure of 1.5 atm a 2) What is the change in internal energy (in u) of system that releases 605.2J of thermal energy to its surroundings and has 229.9cal of work done on it?
Calculate the amount of energy released as heat at constant pressure when 1.00 g of glucose undergoes a combustion reaction according to the equation below: C6H12O6(s) + 6O2(g) ® 6CO2(g) + 6H2O(g) ∆rHϴ = –2806 kJ (A) 16.00 kJ (B) 156.0 kJ (C) 468.0 kJ (D) 2806 kJ (E) 505600 kJ