catement A: Hess' law states that when reactants are converted to products, the change in enthalpy is the ame whether the reaction takes place in one step or in a series of steps. catement B: Hess' law states that if an overall reaction takes place in several steps, its standard reaction nthalpy is the sum of the standard enthalpies of the intermediate reactions, at the same temperature. hich of the following conclusions is correct about statements A and B? O Statement A is correct, Statement B is incorrect. o Both statements are incorrect O Statement A is incorrect, Statement B is correct. O Both statements are correct

catement A: Hess' law states that when reactants are converted to products, the change in enthalpy is the ame whether the reaction takes place in one step or in a series of steps. catement B: Hess' law states that if an overall reaction takes place in several steps, its standard reaction nthalpy is the sum of the standard enthalpies of the intermediate reactions, at the same temperature. hich of the following conclusions is correct about statements A and B? O Statement A is correct, Statement B is incorrect. o Both statements are incorrect O Statement A is incorrect, Statement B is correct. O Both statements are correct

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

app.101edu.co 11. Brightspace Walmart - Hiring Ce... Esc F1 BB 33368 R Q A Z If a system absorbs 155.0 kJ of heat from its surroundings and the system does 45.0 kJ of work on its surroundings, what is the change in the internal energy of the system, in kJ? @ W S F3 X Alt E D C F F6 5 T F7 G B Question 17 of 20 H DELL SE N F10 K M F11 O F12 Alt 1 4 7 +/- PrtScr
Both
A chemist measures the energy change AH during the following reaction: 2 NH,(9) - N,(9)+3H,(9) AH = 160. kJ Use the information to answer the following questions. O endothermic. This reaction is... alo O exothermic. Suppose 46.5 g of NH, react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? O No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Be sure your answer has the correct number of significant digits.
At constant volume, the heat of combustion of a particular compound is -3107.0 kJ/mol. When 1.371 g of this compound (molar mass = 153.31 g/mol) was burned in a bomb calolrimeter, including its contents, rose to 5.685 degrees Celcius. What is the hear capacity (calorimeter constant) of the calorimeter?
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Themeter Mod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 92.55 grams of zinc to 97.73 °C and then drops it into a cup containing 78.30 grams of water at 21.37 °C. She measures the final temperature to be 28.88 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = 3/°C Submit Answer Retry Entire Group 8 more group attempts remaining
Material: Block Mass: Соpper 5.0 g 10.0 g Heating Duration: 2 s Нeat Reset Tinitial T final 20.0 °C 71.9 °C 100 J has been transferred to the block. Experiment Complete Click Reset for a new experiment. Specific heat capacity is a measure of the quantity of heating required to raise 1 g of a substance 1 °C (1 K). Specific heat capacity can be calculated from the equation quantity heating (J) mass (g) x AT(°C) specific heat capacity (J g1 °C) = m x AT Use the following settings: Material: Copper Heating Duration: 2.0 s Block Mass: 5.0 g Run the experiment and calculate the value of the specific heat capacity for copper. ]× Jg°c!
A 21.42g sample of an unknown metal was heated to 99.5ºC, and the added to 50.00g of water contained in a foam coffee cup. The initial temperature of the water was 20.5ºC, and the final temperature of the metal and water was 25.1ºC. The calorimeter constant for the coffee-cup calorimeter was 13.5 J/ºC. What was the specific heat of the metal? * the answer is 0.64 J/gºC, but I need to know how to get there
the formation of table salt from chlorine gas and sodium metal is highly exothermic 2Na + Cl2=NaCl H=-787kJ/mol if I react 35g of sodium, approximately how much heat will e gernerate a). 2400 kJ b).600kJ c). 1200 d). 300 e). 14000
Aluminum mass of metal 50.820g temp of boiling water 98.1 C volume of water in cup 50mL temp of water in cup 21.4 C final temp of system 35.3 C *4.18 J/gK specific heat capacity *Ccal = 16.1 J/C approx. 1. Calculate heat gained by water in calorimeter (qwater) after adding aluminum. 2. Calculate heat gained by calorimeter (qcalorimeter) after adding aluminum. 3. From 1 and 2, calculate heat lost by aluminum (qmetal). 4. Calculate specific heat capacity of aluminum in (J/gK)
6. Toluene, C;Hs, is used in the manufacture of explosives such as TNT. A 1.500 gram sample of liquid toluene was placed in a bomb calorimeter along with excess oxygen. When the combustion of the toluene was initiated, the temperature of the calorimeter rose from 25.000°C to 26.413°C. The products of the reaction were carbon dioxide and water, and the heat capacity of the calorimeter was 45.06 kJ/°c. Write a balanced thermochemical equation for the combustion of toluene.
Topics] [References] Use the References to access important values if needed for this question. A scientist measures the standard enthalpy change for the following reaction to be -754.2 kJ: 2CO(g) + 2NO(g) → 2CO2(g) + N₂ (9) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NO(g) is kJ/mol. $ 4 R Submit Answer F Species AH (kJ/mol) CO₂(g) N₂ (9) 14 V CO(g) %6 5 T G -393.5 0.0 -110.5 Retry Entire Group tv SIA B MacBook Air FO 6 C 9 more group attempts remaining Y H & 7 N F7 U J 8 M DII FO - ( 9 K H lo O I ) O L F10 P A. || : ¡ n F11 Previous + [ command option = 11 1 Next Save and Exit 4) F12 TA delete re