Be sure to answer all parts. Consider the following balanced thermochemical equation for a reaction sometimes...
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. 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?
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3() – MgO(s) + CO2(g) AH = 117.3 kJ (a) Is heat absorbed or released in the reaction? released absorbed (b) What is AHrn for the reverse reaction? (c) What is AH when 3.10 mol of CO2 reacts with ercess Mgo? kJ (d) What is AH when 33.5 g of CO, reacts with excess 190? kJ
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AHrxn - 117.3 kJ (a) Is heat absorbed or released in the reaction? released o absorbed (b) What is AHfor the reverse reaction? (@) What is AH when 4.20 mol of CO, reacts with excess MgO? kJ (d) What is AH when 30.0 g of CO, reacts with excess MgO?
Be sure to answer all parts. When 1 mol of NO(g) forms from its elements, 90.29 kJ of heat is absorbed. (a) Write a balanced thermochemical equation. (Include phases in your equation.) (b) What is AH when 4.02 g of NO decomposes to its elements? kJ
Question 14 5 pts The thermochemical equation for the reaction of nitrogen and hydrogen to form ammonia (NH3) is N2(g) + 3H2(g) -> 2NH3(g) AH = -92.22 kJ What is AH for reaction of 7.183 g of N2 in the above equation? Atomic weights of the elements encountered in this problem are as follows: H 1.00794 g/mol N 14.00674g/mol -47.29 kJ -85.41 kJ -23.65 kJ -68.19 kJ -12.35 kJ
The combination reaction between hydrogen gas and oxygen gas proceeds according to the following balanced thermochemical equation: 2H2(g) + O2(g) +2H200 AH = -572 kJ How much energy in kj is given off when 6.06 grams of hydrogen gas reacts with 400 grams of oxygen gas? 0 -143 1573 0 715 -1716 0 -1573 -858 1716 143 O 858 0 715
help! Be sure to answer all parts. Enter a net ionic equation for the following reaction (including states of matter): CaCl2(aq) + MnSO4(aq) → Write the net ionic equation (including physical states) for the reaction of NaBr(ag) with AgNO3(aq). Click in the answer box to activate the palette. Be sure to answer all parts. Calculate the number of g of o, that will react with 6.28 mol of CzHg. Enter your answer in scientific notation. The balanced equation is: C3Hg(8)...
consider a nypothetical chemical reaction: A+B +C+D (In this equation A, B, C and D stand for some unknown chemical formulas.) Here is an energy diagram for the reaction: 400+ A + B 300+ energy (kJ/mol) 200+ C +D reaction coordinate Use the energy diagram to answer these questions. What is the heat of reaction? kJ/mol Exothermic Is the reaction exothermic or endothermic? Endothermic Can you determine the activation energy? ONeither Yes, it's kJ/mol O No. Yes, it's ] kJ/mol...
1. Consider the following thermochemical equation. NO (g) +O3 (g) → NO2 (g) + O2(g) ΔΗ--1 99 kJ a) This reaction is i. endothermic ii. exothermic b) Calculate the amount of energy (kJ) released when 8.50 g of NO (g) is reacted with an excess of ozone, O3