A 21.0 g sample of pure iron at 85 °C is dropped into 76 g of water at 20. °C. What is the final temperature of the water-iron mixture? The specific heat of water is 4.184 J/g °C. The specific heat of iron is 0.45 J/g °C. Final temperature = °℃ Submit Answer Retry Entire Group 8 more group attempts remaining

Calculate the standard molar enthalpy of formation of NO(g) from the following data: N2(g)+2O22NO2(g)H298=66.4kJ2NO(g)+O22NO2(g)H298=114.1kJ

Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much heat is required to decompose exactly 1 mole of red HgO(s) to Hg(l) and O2(g) under standard conditions?

For the reaction kJ per mole of formed. Calculate the quantity of heat released when 1.00 g of sulfur is burned in oxygen. Calculate the quantity of heat released when 0.501 mole of sulfur is burned in air. i>What quantity of energy is required to break up I mole of into its constituent elements?

The space shuttle Orbiter utilizes the oxidation of methylhydrazine by dinitrogen tetroxide for propulsion: 4N2H3CH3(l)+5N2O4(l)12H2O(g)+9N2(g)+4CO2(g) Calculate H for this reaction

Consider the reaction 2ClF3(g)+2NH3(g)N2(g)+6HF(g)+Cl2(g)H=1196KJ Calculate H for CIF3(g).

What is G for the following reaction? 2Br(aq)+Cl2(g)Br2(l)+2Cl(aq) Use data given in Table 19.1.

The enthalpy change for the reaction of hydrogen gas with fluorine gas (o produce hydrogen fluoride is 542 U for the equation as written: mg src=Images/HTML_99425-10-41QAP_image001.jpg alt="" align="top"/> l type='a'> What is the enthalpy change per mole of hydrogen fluoride produced? Is the reaction exothermic or endothermic as written? What would be the enthalpy change for the reverse of the given equation (that 1%, for the decomposition of HF into its constituent elements)?

How much heat is produced by burning 4.00 moles of acetylene under standard state conditions?

4.60 Why are fuel additives used?