Enthalpy Stoichiometry

Last updated almost 3 years ago

12 questions

Instructions

Give answers in correct significant figures and use unit abbreviations.

Enthalpy Stoichiometry

Last updated almost 3 years ago

12 questions

Instructions

Give answers in correct significant figures and use unit abbreviations.

How much heat will be released when 6.44 g of sulfur reacts with excess oxygen? ΔH = -792 kJ/mol

How much heat will be released when 4.72 g of carbon reacts with excess oxygen? ΔH = -393.5 kJ/mol

How much heat will be absorbed when 38.2 g of bromine reacts with excess H2? ΔH = +72.80 kJ/mol

What mass of propane, C3H8, must be burned to produce 76,000 kJ of energy? ΔH = -2200 kJ/mol

How much heat will be released when 1.48 g of chlorine reacts with excess phosphorus? ΔH = -886 kJ/mol

How much heat will be absorbed when 13.7 g of nitrogen reacts with excess oxygen? ΔH = +180 kJ/mol
N2 + O2 --> 2 NO

What mass of iron must react with excess oxygen in order to produce 3600 kJ of energy? ΔH = -1120 kJ/mol
3Fe + 2O2 --> Fe3O4

How much heat will be released when 12.0 g of H2 reacts with 76.0 g of 02? ΔH = -571.6 kJ/mol

What mass of ammonium nitrate must dissolve in order to absorb 2315 kJ of heat? ΔH = +25.7 kJ/mol
NH4NO3 (s) --> NH4+ (aq) + NO3- (aq)

When 108 g of aluminum reacts with excess chlorine, 2820 kJ of energy is released. Find ΔH for the reaction.

How much energy, in kJ, is released when 5.8 L of C8H18 gas, at STP, combusts in excess oxygen gas? ΔH = -5500 kJ/mol
2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O

Calculate the energy required to allow for the reaction when 10.80 g of N2 reacts with 2.75 L of O2 gas at STP. ΔH = +67.6 kJ/mol (Hint: start with the quantity you have of the LR.)
N2 + O2 --> 2 NO

Enthalpy Stoichiometry

Give answers in correct significant figures and use unit abbreviations.

Enthalpy Stoichiometry

Give answers in correct significant figures and use unit abbreviations.

How much heat will be released when 6.44 g of sulfur reacts with excess oxygen? ΔH = -792 kJ/mol

How much heat will be released when 4.72 g of carbon reacts with excess oxygen? ΔH = -393.5 kJ/mol

How much heat will be absorbed when 38.2 g of bromine reacts with excess H2? ΔH = +72.80 kJ/mol

What mass of propane, C3H8, must be burned to produce 76,000 kJ of energy? ΔH = -2200 kJ/mol

How much heat will be released when 1.48 g of chlorine reacts with excess phosphorus? ΔH = -886 kJ/mol

How much heat will be absorbed when 13.7 g of nitrogen reacts with excess oxygen? ΔH = +180 kJ/molN2 + O2 --> 2 NO

What mass of iron must react with excess oxygen in order to produce 3600 kJ of energy? ΔH = -1120 kJ/mol3Fe + 2O2 --> Fe3O4

How much heat will be released when 12.0 g of H2 reacts with 76.0 g of 02? ΔH = -571.6 kJ/mol

What mass of ammonium nitrate must dissolve in order to absorb 2315 kJ of heat? ΔH = +25.7 kJ/molNH4NO3 (s) --> NH4+ (aq) + NO3- (aq)

When 108 g of aluminum reacts with excess chlorine, 2820 kJ of energy is released. Find ΔH for the reaction.

How much energy, in kJ, is released when 5.8 L of C8H18 gas, at STP, combusts in excess oxygen gas? ΔH = -5500 kJ/mol2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O

Calculate the energy required to allow for the reaction when 10.80 g of N2 reacts with 2.75 L of O2 gas at STP. ΔH = +67.6 kJ/mol (Hint: start with the quantity you have of the LR.)N2 + O2 --> 2 NO

How much heat will be released when 6.44 g of sulfur reacts with excess oxygen? ΔH = -792 kJ/mol

How much heat will be released when 4.72 g of carbon reacts with excess oxygen? ΔH = -393.5 kJ/mol

How much heat will be absorbed when 38.2 g of bromine reacts with excess H2? ΔH = +72.80 kJ/mol

What mass of propane, C3H8, must be burned to produce 76,000 kJ of energy? ΔH = -2200 kJ/mol

How much heat will be released when 1.48 g of chlorine reacts with excess phosphorus? ΔH = -886 kJ/mol

How much heat will be absorbed when 13.7 g of nitrogen reacts with excess oxygen? ΔH = +180 kJ/molN2 + O2 --> 2 NO

What mass of iron must react with excess oxygen in order to produce 3600 kJ of energy? ΔH = -1120 kJ/mol3Fe + 2O2 --> Fe3O4

How much heat will be released when 12.0 g of H2 reacts with 76.0 g of 02? ΔH = -571.6 kJ/mol

What mass of ammonium nitrate must dissolve in order to absorb 2315 kJ of heat? ΔH = +25.7 kJ/molNH4NO3 (s) --> NH4+ (aq) + NO3- (aq)

When 108 g of aluminum reacts with excess chlorine, 2820 kJ of energy is released. Find ΔH for the reaction.

How much energy, in kJ, is released when 5.8 L of C8H18 gas, at STP, combusts in excess oxygen gas? ΔH = -5500 kJ/mol2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O

Calculate the energy required to allow for the reaction when 10.80 g of N2 reacts with 2.75 L of O2 gas at STP. ΔH = +67.6 kJ/mol (Hint: start with the quantity you have of the LR.)N2 + O2 --> 2 NO

How much heat will be absorbed when 13.7 g of nitrogen reacts with excess oxygen? ΔH = +180 kJ/mol
N2 + O2 --> 2 NO

What mass of iron must react with excess oxygen in order to produce 3600 kJ of energy? ΔH = -1120 kJ/mol
3Fe + 2O2 --> Fe3O4

What mass of ammonium nitrate must dissolve in order to absorb 2315 kJ of heat? ΔH = +25.7 kJ/mol
NH4NO3 (s) --> NH4+ (aq) + NO3- (aq)

How much energy, in kJ, is released when 5.8 L of C8H18 gas, at STP, combusts in excess oxygen gas? ΔH = -5500 kJ/mol
2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O

Calculate the energy required to allow for the reaction when 10.80 g of N2 reacts with 2.75 L of O2 gas at STP. ΔH = +67.6 kJ/mol (Hint: start with the quantity you have of the LR.)
N2 + O2 --> 2 NO

How much heat will be absorbed when 13.7 g of nitrogen reacts with excess oxygen? ΔH = +180 kJ/mol
N2 + O2 --> 2 NO

What mass of iron must react with excess oxygen in order to produce 3600 kJ of energy? ΔH = -1120 kJ/mol
3Fe + 2O2 --> Fe3O4

What mass of ammonium nitrate must dissolve in order to absorb 2315 kJ of heat? ΔH = +25.7 kJ/mol
NH4NO3 (s) --> NH4+ (aq) + NO3- (aq)

How much energy, in kJ, is released when 5.8 L of C8H18 gas, at STP, combusts in excess oxygen gas? ΔH = -5500 kJ/mol
2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O

Calculate the energy required to allow for the reaction when 10.80 g of N2 reacts with 2.75 L of O2 gas at STP. ΔH = +67.6 kJ/mol (Hint: start with the quantity you have of the LR.)
N2 + O2 --> 2 NO