Homework 3 • Use standard enthalpies of formation from Table 7.2 to determine the enthalpy change at 25 °C for the following reaction. 2 Cl2(8) + 2H2O(1) –→ 4 HCI(g) + O2(g) AH° = ?

MISSED THIS? Read Section 7.6 (Pages 281- 284), Watch IWE 7.7 View Available Hint(s) Nitromethane (CH,NO2) burns in air to produce significant amounts of heat via the following reaction Hint 1. Calculate the number of moles of nitromethane 2CH,NO, (1) +O2(g)→ 2CO2(g) +3H,O(1) + N2(g) The value of AH is related to the balanced chemical equation by the number of moles of nitromethane. Calculate the number of moles of nitromethane in a 2.73-kg sample. AHn -1418 kJ Express your answer in moles. mol CH, NO2 44.72 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Convert the mass of nitromethane from kg to g. Then use the molar mass of nitromethane as a conversion factor to obtain a value in mol HA Value Units = b

A scientist measures the standard enthalpy change for this reaction to be 296.0 kJ/mol: H₂S(g) + 2 H₂O(l) 3H₂(g) + SO₂(g) Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of H₂S(g) is kJ/mol. Submit Answer Retry Entire Group 1 more group attempt remaining

Q 1 please

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…

a) Using standard enthalpies of formation (in Appendix G in your text), calculate the standard enthalpy change (AH°) for the following reaction shown below. (Show all work.) b) Based on your calculation, is the reaction exothermic or endothermic? 2 H2S(g) + SO2(g) --> 3/8 S8(s) + 2 H20(g)

I need all the answers please

Question 23 please

2 C,H,0(g) + 50,(8) 4 CO2(g) + 4 H,0(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. exothermic Is this reaction exothermic, endothermic, or neither? endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. kJ kJ Calculate the reaction enthalpy AH, per mole of C,H¸0. rxn mol