When 3.0 grams of H2 is reacted with excess C at constant pressure, the reaction forms CH4 and releases 54.2 kJ of heat.
C(s) + 2 H2(g) --> CH4(g)
What is the enthalpy of the reaction in kJ/mol of CH4?
Enter your answer numerically and in terms of kJ/mol.
When 3.0 grams of H2 is reacted with excess C at constant pressure, the reaction forms...
When 3.0 grams of H2 is reacted with excess C at constant pressure, the reaction forms CH4 and releases 54.2 kJ of heat. C(s) + 2 H2(g) --> CH4(g) What is the enthalpy of the reaction in kJ/mol of CH4?
When excess Cl2 at constant pressure reacts with 0.300 mol of CH4(g) 295 kJ of energy evolves. Calculate the value of ΔH for this reaction, as written. CH4(g) + Cl2(g) → CHCl3(l) + H2(g) ΔH = ? a) -1970 kJ b) -1770 kJ c) +1970 kJ d) -983 kJ e) +1770 kJ
For the reaction below, the constant pressure heat of reaction is qp-2451 k] mol at 25 °C. What is the constant volume heat of reaction, qv, at 25 C? 12 CO(g) + 25 H2(g) → C 12H26(I) + 12 H2O(l) Enter your answer in kj mol-1, rounded to the nearest kilojoule. The constant volume heat of reaction is qNumber kJ mol-
Question 15 (1 point) B The reaction of 5.5 grams of HCI with excess NaOH releases 8300 J of heat. What is the molar heat of neutralization. ??, in kJ/mol, for this reaction? Enter your answer with no units. Make sure to indicate the sign (positive or negative). Your Answer: Answer Save
Suppose that 0.490 mol of methane, CH4(g), is reacted with 0.640
mol of fluorine, F2(g), forming CF4(g) and HF(g) as sole products.
Assuming that the reaction occurs at constant pressure, how much
heat is released? Express your answer to three significant figures
and include the appropriate units
Part D Suppose that 0.490 mol of methane, CH4 (g), is reacted with 0.640 mol of fluorine, F2 (g), forming CF4(g) and HF (g) as sole products. Assuming that the reaction occurs at...
1. How much heat is required at constant pressure to melt 1 mole of ice at -25 C to steam at 125° C? boiling point 100c melting point 0.000'C specific heat capacities are gas(steam) 2.08, liquid 4.184 solid (ice) 2.11. All in units of JigC AH(100°C) 40.7 kJ/mol AHu (0.000°C)-6.01 kJ/mol 2. Calculate AHrxn for the reaction: CH4(g)4 Cl2(g) -CC4(g) 4 HCl (g) + Use the following reactions and given AH's: CH4(g) AH =-74.6 kJ 2 H2(g) C(s) C(s)2 Cl2(g)...
Fill in the Blanks For the reaction 4 H2(g) + CO2(g) - CH4(g) + 2 H2O(g) AH--165 kJ a. Is the reaction endothermic or exothermic? b. How many kJ of heat are released when 5.0 moles of CO2 react with excess H2? (Enter a number not words.) c. How many kJ of heat are liberated when 12.9g of H2 react with excess CO2? (Enter a number not words.)
At what temperature will a 13.7 g Cl2 sample exert a pressure of 0.993 bar when confined in a 7.50L container? It is found that 6.00 g of potassium metal reacts with excess water to release 29.8 kJ of heat. This means that, for the reaction: 2K(s) + 2H2O(l) à 2KOH(aq) + H2(g) What is the enthalpy of reaction per mole of potassium metal? 2. The overall reaction in a commercial heat pack can be represented as: 4Fe(s) + 3O2(g)...
Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh out a 0.245 gram piece of metal and combine it with 58.7 mL of 1.00 M HCl in a coffee-cup calorimeter. If the molar mass of the metal is 42.75 g/mol, and you measure that the reaction absorbed 160 J of heat, what is the enthalpy of this reaction in kJ per mole of limiting reactant? Enter your answer numerically to three significant figures...
Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh out a 0.202 gram piece of metal and combine it with 76.3 mL of 1.00 M HCl in a coffee-cup calorimeter. If the molar mass of the metal is 48.37 g/mol, and you measure that the reaction absorbed 121 J of heat, what is the enthalpy of this reaction in kJ per mole of limiting reactant? Enter your answer numerically to three significant figures...