reaction for C,H, is 3) 12 CO, (g) + 6 H,O(1) + 6542 kJ and the heat produced from the burning is added to 5601

According to the reaction below, determine the amount heat (in kJ) that can be generated from the combustion of 1.42 grams of C3H8?   C3H8(g) + 5O2(g) ⟶⟶ 3CO2(g) + 4H2O(g)     Δ?=−2043.2??

2. In studying the energy generated by a person, you may view the person roughly as a constant pressur calorimeter using sugar (i.e., sucrose, C₁2H₂2O11) to generate power. The reaction of table sugar in calorimeter is given by + Ch. 9 Sl....pdf C12H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat. C. a. What is the heat released by consuming one mole of sugar (C₁2H22O11) in this b. Calculate the enthalpy of combustion per sugar utilization. mole Does the result of your calculation make I wi (540 Karak 14 11 M de 2009 1 AP fik Tour of 1 way? 20

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ ((b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =  kJ(c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =   kJ(e) Calculate E when 880.0 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

At constant volume, the heat of combustion of a particular compound, compound A, is −3046.0 kJ/mol.−3046.0 kJ/mol. When 1.753 g1.753 g of compound A (molar mass =112.07 g/mol)=112.07 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.475 ∘C.6.475 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?     Suppose a 3.771 g3.771 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.65 ∘C25.65 ∘C to 29.76 ∘C.29.76 ∘C. What is the heat of combustion per gram of compound B?

4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).

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

Methane (CH4) burns according to the equation CH4 (g) + 2 O2(g) ➞ CO2(g) + 2 H2O(l) with the liberation of 990 kJ per mole of methane reacted. How many grams of oxygen must react with methane in order to release 1780 kJ of energy?

What is the mas of natural gas (CH4) must you burn to emit 276 kJ of heat?