A scientist measures the standard enthalpy change for the following reaction to be -14.6 kJ : Ca(OH)2(aq2 HCl(aq) CaCl2(s) 2 H2O(I) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(aq) is kJ/mol

A chemist measures the enthalpy change AH during the following reaction: Fe(s) + 2 HCl(g) →FeCl₂(s) + H₂(g) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH=157. kJ FeCl₂ (s) + H₂(g) → Fe(s) + 2HC1 (g) 2Fe (s) + 4H C1 (g) 3 FeCl₂ (s) + 3H₂(g) 2FeCl₂ (s) + 2H₂(g) 3Fe (s) + 6HCl (g) ΔΗ [ kJ kJ kJ 0x x10 × Ś

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04

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 -103.2 kJ: 4HCl(g) + O2(g) → 2H₂O(g) + 2Cl₂ (g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(g) is I kJ/mol red Species AH (kJ/mol) H₂O(g) -241.8 Cl₂(g) 0.0 0₂ (9) 0.0

A scientist measures the standard enthalpy change for the following reaction to be -912.5 kJ:2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is  kJ/mol.

Evaporating sweat cools the body because evaporation is an endothermic process: H₂O(1)→ H₂O(g) ▲ Hrxn +44.01 kJ = Part A Estimate the mass of water that must evaporate from the skin to cool the body by 1.20 °C. Assume a body mass of 85.0 kg and assume that the specific heat capacity of the body is 4.00 J/g ° C. Express your answer in grams to three significant figures. m = VE ΑΣΦ ? 8.0 g

A scientist measures the standard enthalpy change for the following reaction to be -679.7 kJ : 2NH3(g) + 2 02(g)N20(g) + 3 H2O(1) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of N20(g) is |kJ/mol.