Given the following thermochemical equation, calculate the amount of heat (in kJ) that is released when 35.0 g of Na2O2 completely react with excess amount of water .
2 Na2O2 (s) + 2 H2O (l) → 4 NaOH (aq) + O2 (g) Δ H = - 126 kJ
Number of moles of Na2O2 = 35.0 g / 77.98 g/mol = 0.449 mole
From the balanced equation we can say that
2 mole of Na2O2 produces 126 kJ of heat so
0.449 mole of Na2O2 will produce
= 0.449 mole of Na2O2 *(126 kJ of heat / 2 mole of Na2O2)
= 28.3 kJ of heat
Therefore, the amount of heat produced would be 28.3 kJ
Given the following thermochemical equation, calculate the amount of heat (in kJ) that is released when...
How much Na2O2 would need to react in order to release 1000 kJ of heat? Show your work. 2 Na2O2 (s) + 2 H2O (l) ---> 4NaOH (aq) + O2 (g) Delta Hrxn = -126 kJ
Use the following thermochemical equation to calculate how much heat in kilojoules is evolved or absorbed when 14.4g of liquid water are converted to hydrogen and oxygen gas. 2H2(g) + O2(g) -----> 2H2O (l)Delat H°= -571.6 kJ
The thermochemical equation for the combustion of propane is: C3H8 (g) + 5 O2 (g) 3 CO2 (g) + 4 H2O (l) H = -2220 kJ What is the enthalpy change when 35.0 g of propane react?
How much heat is absorbed/released when 20.00 g of NH3(g) reacts in the presence of excess O2 (g) to produce NO (g) and H2O (l) according to the following chemical equation? 4NH3 (g) + 5O2 (g) ---> 4NO (g) +6H2O (l) Δ H: +1168 kJ a. 342.9 kJ of heat are absorbed. b. 342.9 kJ of heat are released. c. 1372 kJ of heat are absorbed. d. 1372 kJ of heat are released. Please explain your answer.
When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)Δ?=−764 kJ How much methanol, in grams, must be burned to produce 807 kJ of heat? mass in grams:
1. What is the change in internal energy of a system that does 7.02 kJ of work and absorbs 888 J of heat? 2. Given the reaction 2 Na2O2(g) + 2 H2O(l) → 4 NaOH(s) + O2(g) ∆H = -109 kJ determine ∆H for the following reactions. a)16 Na2O2(g) + 16 H2O(l) → 32 NaOH(s) + 8 O2(g) b)2 NaOH(s) + ½ O2(g) → Na2O2(s) + H2O(l) please make it in word software
The following thermochemical equation is for the reaction of carbon monoxide(g) with water(l) to form carbon dioxide(g) and hydrogen(g). CO(g) + H2O(l) CO2(g) + H2(g) H = 2.80 kJ When 9.83 grams of carbon monoxide(g) react with excess water(l),_______________ kJ of energy are___________ ( absorbed or evolved ) .
1. The heat capacity of a calorimeter is given as 1264 J/oC. Suppose the enthalpy of solution for calcium chloride (MM=111 g/mol) in water is given by the thermochemical equation: CaCl2(s) + H2O(l) → Ca2+(aq) + 2Cl-(aq) ΔH = -81.0 kJ/mol. Calculate the temperature change if 11.1 g of calcium chloride is dissolved in water in the calorimeter. 2. Given the following data, calculate ΔH for the reaction of two moles of carbon monoxide with oxygen gasto give carbon dioxide....
Calculate ΔH for the following reaction, CaO(s) + CO2(g) → CaCO3(s) given the thermochemical equations below. 2 Ca(s) + O2(g) → 2 CaO(s) ΔH = -1270.2 kJ C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ 2 Ca(s) + 2 C(s) + 3 O2(g) → 2 CaCO3(s) ΔH = -2413.8 kJ A compound contains C, H and O as the elements. A 20.0 g-sample is comprised of 1.34 g H and also 8.00 g of C. What...
The thermochemical equation of combustion of methane is: CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l) ΔΗ =-890.3 kJ 1. Calculate the AH when 5.00 g CH4 react with excess of oxygen. 2. Calculate AH when 2L CH4 at 49 °C and 782 mmHg react with an excess of oxygen 3. Calculate AH when 2L CH4 react with L O2 in a reaction vessel kept at 49 °C and 782 mmHg.