Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic     (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. H =   kJ (c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?   g (d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure? H =   kJ

The reaction between HCl and NaOH is represented below. When equal volumes of 1.00 M NaOH and 1.00 M HCl are mixed, 57.1 kJ of heat is released. What would A H be if 2.00 M HCI and 2.00 M NaOH is used instead of 1.00 M? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) AH = -57.1 kJ/mol... (A) - 28.6 kJ B-85.7 kJ (c) -57.1 kJ D - 114 kJ

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When 0.617 g of sodium metal is added to an excess of hydrochloric acid, 6410 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCl(aq) - Enthalpy of reaction: 2 NaCl(aq) + H₂(g) kJ

How much heat (in kJ) is evolved (under standard conditions) when 97.55 g of copper reacts to form copper (II) oxide?

The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol

Calculate AH for the reaction P4010(s) + 6PC15(g) – 10C13PO(g) given, P4(s) + 6C12(g) → 4PC13(g) AH = -1225.6 kJ P4(s) + 502(g) – P4010(s) AH = -2967.3 kJ PC13(g) + Cl2(g) → PC15(g) AH = -84.2 kJ PC13(g) + (1/2)02(g) – C13PO(g) AH=-285.7 kJ ΔΗ- kJ

CH3OH(g)  CO(g) + 2 H2(g)   H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic    (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = ____kJ(c) If the enthalpy change is 18.0 kJ, how many grams of hydrogen gas are produced?____g(d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = ____kJ(e) Calculate E when 750.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K _____kJ HopHelpCh5N1

Which of the reactions are exothermic?

Consider the following chemical reaction: What is AH for the following reaction? 2Mg(s) + O₂(g) → 2MgO(s); AH = -1204KJ 4MgO 4Mg(s) + 20₂(g); AH =