According to the following thermochemical equation, what mass of H2O (in g) must form in order...
According to the following thermochemical equation, what mass of
H2O (in g) must form in order to produce 975 kJ of
energy?
SiO2(s) + 4 HF(g) → SiF4(g) + 2
H2O(l) ΔH°rxn = -184 kJ
|
54.1 g |
||
|
95.5 g |
||
|
102 g |
||
|
68.0 g |
||
|
191 g |
Homework Answers
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According to the following thermochemical equation, what mass of
H2O (in g) must form in order...
QUESTION 1 According to the following thermochemical equation, what mass of HF (in g) must react...
QUESTION 1 According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4 HF(g) SiF4(g) + 2 H20) AH®rxn = -184 kJ 1079 150.9 173 g 37.59 QUESTION 2 The value of AH® for the reaction below is -1107 kJ: 2Ba (s) + O2(g) + 2Bao (s) How many kJ of heat are released when 5.75 g of Bao (s) is produced? 96.3...
can you do all of them please 4 Using the following thermochemical equation, determine the amount...
can you do all of them please
4 Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6()+15 02(g)12 CO2(g ) + 6 H20(g) A) 1.43 x 105 kl/kg CO2 B) 2.30x 104 kl/kg CO2 AH"xn-6278 kJ C) 4.34 x 104 kl/kg CO2 D) 1.19x 104 kl/kg CO2 E) 8.40x 105 kl/kg CO2 48) Using the following equation for the combustion of octane, calculate the amount...
The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium...
The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium chloride(s). HCI(g) + NH3(g) NH CH) AH = -176 kJ/mol-rxn How many grams of HCI(g) would have to react to produce 51.9 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen bromide(r) with chlorine() to form hydrogen chloride) and bromine(g) 2HBr(g) + Cl2(g) +2HCl(g) + Brz(8) AH = -81.1 kJ/mol-rxn When 16.4 grams of hydrogen bromide(g) react with excess...
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g)...
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g) 2H2O(g) AH=-484 kJ How many grams of H2(g) would have to react to produce 61.5 kJ of energy? grams
The propane fuel (C3H8) used in gas barbeques burns according to this thermochemical equation. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2044kJ If...
The propane fuel (C3H8) used in gas barbeques burns according to this thermochemical equation. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2044kJ If a pork roast must absorb 1.7×103 kJ to fully cook, and if only 15 % of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g)...
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
The following thermochemical equation is for the reaction of carbon monoxide(g) with water(l) to form carbon...
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 ) .
The propane fuel (C3H8) used in gas barbeques burns according to the following thermochemical equation: C3H8(g)+5O2(g)...
The propane fuel (C3H8) used in gas barbeques burns according to the following thermochemical equation:C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) ΔH rxn= 2217kJPart AIf a pork roast must absorb 1500kJ to fully cook, and if only 12% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?Express your answer using two significant figures. m=_____________________g
Octane (C8H18) is a component of gasoline that burns according to the following equation: C8H18(l)+252O2(g)→8CO2(g)+9H2O(g) ΔH∘rxn=−5074.1kJ...
Octane (C8H18) is a component of gasoline that burns according to the following equation: C8H18(l)+252O2(g)→8CO2(g)+9H2O(g) ΔH∘rxn=−5074.1kJ What mass of octane (in g ) is required to produce 1850 kJ of heat?
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and...
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
QUESTION 1 According to the following thermochemical equation, what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4 HF(g) SiF4(g) + 2 H20) AH®rxn = -184 kJ 1079 150.9 173 g 37.59 QUESTION 2 The value of AH® for the reaction below is -1107 kJ: 2Ba (s) + O2(g) + 2Bao (s) How many kJ of heat are released when 5.75 g of Bao (s) is produced? 96.3...
can you do all of them please
4 Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6()+15 02(g)12 CO2(g ) + 6 H20(g) A) 1.43 x 105 kl/kg CO2 B) 2.30x 104 kl/kg CO2 AH"xn-6278 kJ C) 4.34 x 104 kl/kg CO2 D) 1.19x 104 kl/kg CO2 E) 8.40x 105 kl/kg CO2 48) Using the following equation for the combustion of octane, calculate the amount...
The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium chloride(s). HCI(g) + NH3(g) NH CH) AH = -176 kJ/mol-rxn How many grams of HCI(g) would have to react to produce 51.9 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen bromide(r) with chlorine() to form hydrogen chloride) and bromine(g) 2HBr(g) + Cl2(g) +2HCl(g) + Brz(8) AH = -81.1 kJ/mol-rxn When 16.4 grams of hydrogen bromide(g) react with excess...
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g) 2H2O(g) AH=-484 kJ How many grams of H2(g) would have to react to produce 61.5 kJ of energy? grams
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
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