Be sure to answer all parts. When 1 mol of NO(g) forms from its elements, 90.29...
Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AH - 117.3 kJ (a) Is heat absorbed or released in the reaction? absorbed released (b) What is A n for the reverse reaction? -1173 EJ (c) What is AH when 5.20 mol of CO, reacts with excess Mgo? (a) What is AH when 32.5 g of CO, reacts with exces: Mgo?
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H2S production: =Sg(s) + H2(g) → H2S() AH rxn = -20.2 kJ his an exothermic or endothermic reaction? endothermic exothermic (b) What is AH rxn for the reverse reaction? KJ (c) What is AH when 3.10 mol of Sg reacts? kJ
Be sure to answer all parts. A mercury mirror forms inside a test tube as a result of the thermal decomposition of mercury(II) oxide: 2 HgO(s) → 2 Hg(1) + O2(g) AH rxn = 181.6 kJ (a) How much heat is needed to decompose 687 g of the oxide? I kJ (b) If 631 kJ of heat is absorbed, how many grams of Hg form? 00 (Enter your answer in scientific notation.)
Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes used for H,S production: (BH-H+ (a) Is this an exothermic or endothermic reaction? AH--20.2kJ endothermic exothermic (b) What is AH for the reverse reaction? kJ (c) What is AH when 4.30 mol of Ss reacts? kJ draw HIR < Prey 10 of 16 Ne: hp
Part A: Write an equation for the formation of NO(g) from its elements in their standard states. Express your answer as a chemical equation. Identify all of the phases in your answer. Part B: Write an equation for the formation of BF3(g) from its elements in their standard states. Express your answer as a chemical equation. Identify all of the phases in your answer. Part C: Write an equation for the formation of C6H6(l) from its elements in their standard...
html Saved 10 attempts left Check my work Be sure to answer all parts. Determine the amount of heat (in kJ) associated with the production of L46 x 10g of NO, according to- the following equation: 2 NOg)+O2)2NO (g) Enter your answer in scientific notation. AH--114.6 kJ/mol x 10 kJ 2 of 2 <Prev search
Be sure to answer all parts. Mass and energy are alternate forms of a single entity called mass-energy. The relationship between these two physical quantities is described by Einstein's equation, E = mc², where Els energy, mis mass, and c is the speed of light (3.00 x 108 m/s). In a combustion experiment, it was found that 12.096 g of hydrogen molecules combined with 96.000 g of oxygen molecules to form water and released 1.715 10 kJ of heat. Calculate...
Be sure to answer all parts. Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe2O3) is: 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) AH --1.65 x 103 kJ (a) What is the Ahr when 0.250 kg of iron rusts? x 10 kJ (b) How much rust forms when 2.90 x 109 kJ of heat is...
Be sure to answer all parts. Calculate the magnitude of q for a system that does 688000 kJ of work on its surroundings and for which the change in total internal energy is -6500 kJ. x 10 kJ (Enter your answer in scientific notation.) Indicate whether heat is absorbed or released by the system. heat is absorbed heat is released
6. When a student dissolves 41.41grams of NaNO, in 300. g. of water at 24.11 deg. C, 10.0 kJ of her are are absorbed from the water. a. what is the q for the water? b. what is the AH for the solution process in kJ/mol? c. Write a balanced equation and use Hess's Law to determine the theoretical heat of solution in kJ/m