kJ

The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) What mass of aluminum is needed to produce 664. kJ of heat ? AH = -850. kJ O 36.7 g O 31.3 g O 32.8 g O 55.3 g 42.2g • Previous Not saved MacBook Air 吕0 F1 F2 DII

In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH)₂ was added to 70.0 mL of 0.600 M HC1. The reaction caused the temperature of the solution to rise from 23.98 °C to 28.07 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184J/g °C.) respectively), what is AH for this reaction (per mole H₂O produced)? Assume that the total volume is the sum of the individual volumes. ΔΗ = 2.396 Incorrect kJ/mol H₂O

Determine the enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s) (Please show steps)

Consider the hypothetical thermochemical equation 3 A + B → 2 C for which ΔH = 58.7 kJ/mol. If the reaction absorbs 345 kJ of heat, What quantity in moles of C would be produced?

The complete combustion of propane, C 3H 8(g), is represented by the equation: C 3H 8(g) + 5 O 2(g) → 3 CO 2(g) + 4 H 2O(l) Δ H° = -2220 kJ How much heat is evolved in the complete combustion of 2.50 g C 3H 8(g)?

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.19 kg sample of C,H,N from -4.5 °C to 6.6 °C. The experiment shows that 6.14 × 10° J of heat are needed. What can the chemist report for the molar heat capacity of C,H,N? Round your answer to 2 significant digits. O J-mol -1 - 1 ·K х10 ?

For the highly exothermic reaction H2(g) + 1/2 O2(g) → H2O(g) qrx =DHrx = -242 kJ, What quantity of heat (kJ) is exchanged when 17.9 moles of hydrogen and 1.13 moles of oxygen are combusted?

In the following reaction, what is the quantity of heat (in kJ) released when 3.91 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO₂ (g) + 2 H₂O(g) AH° = -802 kJ/mol -

Consider the following equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover. C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g) ΔHrxn=−1790kJ if a bottle of nail polish remover contains 161  g  of acetone, how much heat would be released by its complete combustion?