Question 1

Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below?
H2(g) + 2(g) +   O2(g) → H2O(l) ; ΔH = -285.8 kJ A) Per mole of O2,the change in enthalpy is -571.6 kJ. B) The value -571.6 kJ pertains to 1 mol of liquid water. C) If the equation is reversed,ΔH becomes +285.8 kJ. D) If the equation is multiplied by 2,ΔH becomes -571.6 kJ. E) For the reaction H2(g) +   O2(g) → H2O(g) ,ΔH is not equal to -285.8 kJ." class="answers-bank-image d-inline" rel="preload" >
O2(g) → H2O(l) ; ΔH = -285.8 kJ

Accepted Answer

A)  Per mole of O2,the change in enthalpy is -571.6 kJ.
B)  The value -571.6 kJ pertains to 1 mol of liquid water.
C)  If the equation is reversed,ΔH becomes +285.8 kJ.
D)  If the equation is multiplied by 2,ΔH becomes -571.6 kJ.
E)  For the reaction H2(g) + 2(g) +   O2(g) → H2O(l) ; ΔH = -285.8 kJ 
A)  Per mole of O2,the change in enthalpy is -571.6 kJ. 
B)  The value -571.6 kJ pertains to 1 mol of liquid water. 
C)  If the equation is reversed,ΔH becomes +285.8 kJ. 
D)  If the equation is multiplied by 2,ΔH becomes -571.6 kJ. 
E)  For the reaction H2(g) +   O2(g) → H2O(g) ,ΔH is not equal to -285.8 kJ." class="answers-bank-image d-inline" rel="preload" > O2(g) → H2O(g) ,ΔH is not equal to -285.8 kJ.

Question 2

At constant pressure,the sign of q for the process CO2(s) → CO2(g) is expected to be

Accepted Answer

A)  positive,and the process is exothermic.
B)  negative,and the process is exothermic.
C)  impossible to predict.
D)  positive,and the process is endothermic.
E)  negative,and the process is endothermic.

Question 3

What is ΔH° for the following reaction?
2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) 
Substance
ΔH°f (kJ/mol) 
C2H2(g) 
+226.7
CO2(g) 
-393.5
H2O(l) 
-285.8

Accepted Answer

A)  +1692.2 kJ
B)  -452.6 kJ
C)  -1692.2 kJ
D)  +2599.0 kJ
E)  -2599.0 kJ

Question 4

From the following information,determine the enthalpy of formation of C2H4(g) . 2H4(g) .   C2H4(g) → C(s) + H2(g) ; ΔH = -26.2 kJ A) -26.2 kJ/mol B) 26.2 kJ/mol C) 104.8 kJ/mol D) -52.4 kJ/mol E) 52.4 kJ/mol" class="answers-bank-image d-inline" rel="preload" > C2H4(g) → C(s) + H2(g) ; ΔH = -26.2 kJ

Accepted Answer

A)  -26.2 kJ/mol
B)  26.2 kJ/mol
C)  104.8 kJ/mol
D)  -52.4 kJ/mol
E)  52.4 kJ/mol

Question 5

Two metals of equal mass with different heat capacities are subjected to the same amount of heat.Which undergoes the smaller change in temperature?

Accepted Answer

A)  The metal with the higher heat capacity undergoes the smaller change in temperature.
B)  Both undergo the same change in temperature.
C)  You need to know the initial temperatures of the metals.
D)  You need to know which metals you have.
E)  The metal with the lower heat capacity undergoes the smaller change in temperature.

Question 6

The balanced equation representing the standard enthalpy of formation reaction for NH3(g) is

Accepted Answer

A)  N(g) + 3(g) is 
A)  N(g) +   H2(g) → NH3(g) . 
B)     N2(g) + 3H(g) → NH3(g) . 
C)  N(g) + 3H(g) → NH3(g) . 
D)     N2(g) +   H2(g) → NH3(g) . 
E)  N2(g) + H2(g) → NH3(g) ." class="answers-bank-image d-inline" rel="preload" > H2(g) → NH3(g) .
B)   3(g) is 
A)  N(g) +   H2(g) → NH3(g) . 
B)     N2(g) + 3H(g) → NH3(g) . 
C)  N(g) + 3H(g) → NH3(g) . 
D)     N2(g) +   H2(g) → NH3(g) . 
E)  N2(g) + H2(g) → NH3(g) ." class="answers-bank-image d-inline" rel="preload" > N2(g) + 3H(g) → NH3(g) .
C)  N(g) + 3H(g) → NH3(g) .
D)   3(g) is 
A)  N(g) +   H2(g) → NH3(g) . 
B)     N2(g) + 3H(g) → NH3(g) . 
C)  N(g) + 3H(g) → NH3(g) . 
D)     N2(g) +   H2(g) → NH3(g) . 
E)  N2(g) + H2(g) → NH3(g) ." class="answers-bank-image d-inline" rel="preload" > N2(g) + 3(g) is 
A)  N(g) +   H2(g) → NH3(g) . 
B)     N2(g) + 3H(g) → NH3(g) . 
C)  N(g) + 3H(g) → NH3(g) . 
D)     N2(g) +   H2(g) → NH3(g) . 
E)  N2(g) + H2(g) → NH3(g) ." class="answers-bank-image d-inline" rel="preload" > H2(g) → NH3(g) .
E)  N2(g) + H2(g) → NH3(g) .

Question 7

How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts with 29.0 L of carbon dioxide gas,measured at 1.00 atm pressure and 25.0°C? (R = 0.0821 L • atm/(K • mol) ) 
CaO(s) + CO2(g) → CaCO3(s) ; ΔH° = -178.3 kJ

Accepted Answer

A)  -3.11 × 102 kJ
B)  -1.74 × 104 kJ
C)  -5.22 × 102 kJ
D)  -2.11 × 102 kJ
E)  -5.17 × 103 kJ

Question 8

What is the kinetic energy of a 2000-lb car traveling at 59 miles per hour? (1 lb = 0.4536 kg,1 mi = 1.609 km)

Accepted Answer

A)  3.2 × 10-7 J
B)  1.5 × 106 J
C)  5.3 × 1019 J
D)  3.2 × 105 J
E)  4.7 × 10-8 J

Question 9

The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid calcium nitrate,Ca(NO3) 2?

Accepted Answer

A)  Ca2+(g) + 2NO3-(g) → Ca(NO3) 2(s) 
B)  Ca(s) + N2(g) + 3O2(g) → Ca(NO3) 2(s) 
C)  Ca(g) + 2N(g) + 6O(g) → Ca(NO3) 2(s) 
D)  Ca(s) + N2(g) + 2O3(g) → Ca(NO3) 2(s) 
E)  Ca2+(aq) + 2NO3-(aq) → Ca(NO3) 2(s)

Question 10

Which of the following statements is incorrect?

Accepted Answer

A)  Internal energy is a state function.
B)  The value of q is positive when heat flows into a system from the surroundings.
C)  The value of q is positive in an endothermic process.
D)  Heat flows from a system into the surroundings in an endothermic process.
E)  Enthalpy is a state function.

Question 11

Given:
4AlCl3(s) + 3O2(g) → 2Al2O3(s) + 6Cl2(g) ; ΔH = -529.0 kJ
Determine ΔH for the following thermochemical equation.
Cl2(g) +3(s) + 3O2(g) → 2Al2O3(s) + 6Cl2(g) ; ΔH = -529.0 kJ Determine ΔH for the following thermochemical equation. Cl2(g) +  Al2O3(s) →  AlCl3(s) + O2(g)  A) +264.5 kJ B) +529.0 kJ C) +88.2 kJ D) +176.3 kJ E) -176.3 kJ" class="answers-bank-image d-inline" rel="preload" > Al2O3(s) → 3(s) + 3O2(g) → 2Al2O3(s) + 6Cl2(g) ; ΔH = -529.0 kJ Determine ΔH for the following thermochemical equation. Cl2(g) +  Al2O3(s) →  AlCl3(s) + O2(g)  A) +264.5 kJ B) +529.0 kJ C) +88.2 kJ D) +176.3 kJ E) -176.3 kJ" class="answers-bank-image d-inline" rel="preload" >AlCl3(s) +3(s) + 3O2(g) → 2Al2O3(s) + 6Cl2(g) ; ΔH = -529.0 kJ Determine ΔH for the following thermochemical equation. Cl2(g) +  Al2O3(s) →  AlCl3(s) + O2(g)  A) +264.5 kJ B) +529.0 kJ C) +88.2 kJ D) +176.3 kJ E) -176.3 kJ" class="answers-bank-image d-inline" rel="preload" >O2(g)

Accepted Answer

A)  +264.5 kJ
B)  +529.0 kJ
C)  +88.2 kJ
D)  +176.3 kJ
E)  -176.3 kJ

Question 12

Consider the following changes at constant temperature and pressure:
H2O(s) → H2O(l) ; ΔH1
H2O(l) → H2O(g) ; ΔH2
H2O(g) → H2O(s) ; ΔH3
Using Hess's law,the sum ΔH1 + ΔH2 + ΔH3 is

Accepted Answer

A)  equal to zero.
B)  sometimes greater than zero and sometimes less than zero.
C)  less than zero.
D)  cannot be determined without numerical values for ΔH.
E)  greater than zero.

Question 13

For which of the following equations is the enthalpy change at 1 atm pressure equal to the standard enthalpy of formation of liquid formic acid,HCOOH?

Accepted Answer

A)  C(g) + 2H(g) + 2O(g) → HCOOH(l) 
B)  C(s) + 2H(g) + 2O(g) → HCOOH(l) 
C)  C(s) + H2(g) + O2(g) → HCOOH(l) 
D)  CO(g) + H2O(l) → HCOOH(l) 
E)  CO2(g) + H2(g) → HCOOH(l)

Question 14

A 100 g sample of each of the following metals is heated from 35°C to 45°C.Which metal absorbs the lowest amount of heat energy?
Metal
Specific Heat
Copper
0) 385 J/(g ∙ °C) 
Magnesium
1) 02 J/(g ∙ °C) 
Mercury
0) 138 J/(g ∙ °C) 
Silver
0) 237 J/(g ∙ °C) 
Lead
0) 129 J/(g ∙ °C)

Accepted Answer

A)  lead
B)  magnesium
C)  silver
D)  mercury
E)  copper

Question 15

The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid potassium bromate,KBrO3?

Accepted Answer

A)  K(s) + Br(g) + 3O(g) → KBrO3(s) 
B)  K(g) + Br(g) + 3O(g) → KBrO3(s) 
C)  K(g) + 3? 
A)  K(s) + Br(g) + 3O(g) → KBrO3(s)  
B)  K(g) + Br(g) + 3O(g) → KBrO3(s)  
C)  K(g) +   Br2(g) +   O2(g) → KBrO3(s)  
D)  K(s) +   Br2(l) +   O2(g) → KBrO3(s)  
E)  K(s) +   Br2(g) +   O2(g) → KBrO3(s) " class="answers-bank-image d-inline" rel="preload" > Br2(g) + 3? 
A)  K(s) + Br(g) + 3O(g) → KBrO3(s)  
B)  K(g) + Br(g) + 3O(g) → KBrO3(s)  
C)  K(g) +   Br2(g) +   O2(g) → KBrO3(s)  
D)  K(s) +   Br2(l) +   O2(g) → KBrO3(s)  
E)  K(s) +   Br2(g) +   O2(g) → KBrO3(s) " class="answers-bank-image d-inline" rel="preload" > O2(g) → KBrO3(s) 
D)  K(s) + 3? 
A)  K(s) + Br(g) + 3O(g) → KBrO3(s)  
B)  K(g) + Br(g) + 3O(g) → KBrO3(s)  
C)  K(g) +   Br2(g) +   O2(g) → KBrO3(s)  
D)  K(s) +   Br2(l) +   O2(g) → KBrO3(s)  
E)  K(s) +   Br2(g) +   O2(g) → KBrO3(s) " class="answers-bank-image d-inline" rel="preload" > Br2(l) + 3? 
A)  K(s) + Br(g) + 3O(g) → KBrO3(s)  
B)  K(g) + Br(g) + 3O(g) → KBrO3(s)  
C)  K(g) +   Br2(g) +   O2(g) → KBrO3(s)  
D)  K(s) +   Br2(l) +   O2(g) → KBrO3(s)  
E)  K(s) +   Br2(g) +   O2(g) → KBrO3(s) " class="answers-bank-image d-inline" rel="preload" > O2(g) → KBrO3(s) 
E)  K(s) + 3? 
A)  K(s) + Br(g) + 3O(g) → KBrO3(s)  
B)  K(g) + Br(g) + 3O(g) → KBrO3(s)  
C)  K(g) +   Br2(g) +   O2(g) → KBrO3(s)  
D)  K(s) +   Br2(l) +   O2(g) → KBrO3(s)  
E)  K(s) +   Br2(g) +   O2(g) → KBrO3(s) " class="answers-bank-image d-inline" rel="preload" > Br2(g) + 3? 
A)  K(s) + Br(g) + 3O(g) → KBrO3(s)  
B)  K(g) + Br(g) + 3O(g) → KBrO3(s)  
C)  K(g) +   Br2(g) +   O2(g) → KBrO3(s)  
D)  K(s) +   Br2(l) +   O2(g) → KBrO3(s)  
E)  K(s) +   Br2(g) +   O2(g) → KBrO3(s) " class="answers-bank-image d-inline" rel="preload" > O2(g) → KBrO3(s)

Question 16

Exactly 209.2 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C.What is the specific heat capacity of the metal?

Accepted Answer

A)  0.598 J/(g ∙ °
C)  
B)  1.67 J/(g ∙ °
C)  
C)  14.7 J/(g ∙ °
C)  
D)  50.0 J/(g ∙ °
C)  
E)  none of these

Question 17

The reaction of iron with hydrochloric acid is represented by the following thermochemical equation.
Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g) ; ΔH° = -87.9 kJ
How much heat is liberated at constant pressure if 0.154 g of iron reacts with 25.7 mL of 0.358 M HCl?

Accepted Answer

A)  1.85 kJ
B)  13.5 kJ
C)  0.242 kJ
D)  0.404 kJ
E)  87.9 kJ

Question 18

What is the standard enthalpy change for the combustion of gaseous propylene,C3H6?
C3H6(g) + 3H6? C3H6(g) +   O2(g) → 3CO2(g) + 3H2O(l)  Substance ΔH°f (kJ/mol)  C3H6(g)  +20) 4 CO2(g)  -393.5 H2O(l)  -285.8 A) +2017.5 kJ B) -2058.3 kJ C) -658.9 kJ D) -2017.5 kJ E) +2058.3 kJ" class="answers-bank-image d-inline" rel="preload" >
O2(g) → 3CO2(g) + 3H2O(l) 
Substance
ΔH°f (kJ/mol) 
C3H6(g) 
+20) 4
CO2(g) 
-393.5
H2O(l) 
-285.8

Accepted Answer

A)  +2017.5 kJ
B)  -2058.3 kJ
C)  -658.9 kJ
D)  -2017.5 kJ
E)  +2058.3 kJ

Question 19

Given the thermochemical equation
2Al(s) + 2(g) → Al2O3(s) ; ΔH = -1676 kJ Find ΔH for the following reaction. 2Al2O3(s) → 4Al(s) + 3O2(g)  A) 838 kJ B) 1676 kJ C) -1676 kJ D) 3352 kJ E) -838 kJ" class="answers-bank-image d-inline" rel="preload" >
O2(g) → Al2O3(s) ; ΔH = -1676 kJ
Find ΔH for the following reaction.
2Al2O3(s) → 4Al(s) + 3O2(g)

Accepted Answer

A)  838 kJ
B)  1676 kJ
C)  -1676 kJ
D)  3352 kJ
E)  -838 kJ

Question 20

How much heat is evolved upon the complete oxidation of 6 g of aluminum at 25°C and 1 atm pressure? ( 2O3 is -1676 kJ/mol.)  4Al(s) + 3O2(g) → 2Al2O3(s)  A) 9.238 × 103 kJ B) 342.3 kJ C) 684.7 kJ D) 171.1 kJ E) 85.59 kJ" class="answers-bank-image d-inline" rel="preload" > for Al2O3 is -1676 kJ/mol.) 
4Al(s) + 3O2(g) → 2Al2O3(s)

Accepted Answer

A)  9.238 × 103 kJ
B)  342.3 kJ
C)  684.7 kJ
D)  171.1 kJ
E)  85.59 kJ

Exam 6: Thermochemistry

The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid potassium bromate,KBrO3?

Correct AnswerverifiedShow Answer

What is the standard enthalpy change for the combustion of gaseous propylene,C3H6? C3H6(g) + O2(g) → 3CO2(g) + 3H2O(l) Substance ΔH°f (kJ/mol) C3H6(g) +20) 4 CO2(g) -393.5 H2O(l) -285.8

Correct AnswerverifiedShow Answer

What is the kinetic energy of a 2000-lb car traveling at 59 miles per hour? (1 lb = 0.4536 kg,1 mi = 1.609 km)

Correct AnswerverifiedShow Answer

For which of the following equations is the enthalpy change at 1 atm pressure equal to the standard enthalpy of formation of liquid formic acid,HCOOH?

Correct AnswerverifiedShow Answer

At constant pressure,the sign of q for the process CO2(s) → CO2(g) is expected to be

Correct AnswerverifiedShow Answer

Two metals of equal mass with different heat capacities are subjected to the same amount of heat.Which undergoes the smaller change in temperature?

Correct AnswerverifiedShow Answer

From the following information,determine the enthalpy of formation of C2H4(g) . C2H4(g) → C(s) + H2(g) ; ΔH = -26.2 kJ

Correct AnswerverifiedShow Answer

How much heat is evolved upon the complete oxidation of 6 g of aluminum at 25°C and 1 atm pressure? ( for Al2O3 is -1676 kJ/mol.) 4Al(s) + 3O2(g) → 2Al2O3(s)

Correct AnswerverifiedShow Answer

Given: 4AlCl3(s) + 3O2(g) → 2Al2O3(s) + 6Cl2(g) ; ΔH = -529.0 kJ Determine ΔH for the following thermochemical equation. Cl2(g) + Al2O3(s) → AlCl3(s) +O2(g)

Correct AnswerverifiedShow Answer

Consider the following changes at constant temperature and pressure: H2O(s) → H2O(l) ; ΔH1 H2O(l) → H2O(g) ; ΔH2 H2O(g) → H2O(s) ; ΔH3 Using Hess's law,the sum ΔH1 + ΔH2 + ΔH3 is

Correct AnswerverifiedShow Answer

Which of the following statements is incorrect?

Correct AnswerverifiedShow Answer

Exactly 209.2 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C.What is the specific heat capacity of the metal?

Correct AnswerverifiedShow Answer

How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts with 29.0 L of carbon dioxide gas,measured at 1.00 atm pressure and 25.0°C? (R = 0.0821 L • atm/(K • mol) ) CaO(s) + CO2(g) → CaCO3(s) ; ΔH° = -178.3 kJ

Correct AnswerverifiedShow Answer

The balanced equation representing the standard enthalpy of formation reaction for NH3(g) is

Correct AnswerverifiedShow Answer

What is ΔH° for the following reaction? 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) Substance ΔH°f (kJ/mol) C2H2(g) +226.7 CO2(g) -393.5 H2O(l) -285.8

Correct AnswerverifiedShow Answer

Given the thermochemical equation 2Al(s) + O2(g) → Al2O3(s) ; ΔH = -1676 kJ Find ΔH for the following reaction. 2Al2O3(s) → 4Al(s) + 3O2(g)

Correct AnswerverifiedShow Answer

The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid calcium nitrate,Ca(NO3) 2?

Correct AnswerverifiedShow Answer

A 100 g sample of each of the following metals is heated from 35°C to 45°C.Which metal absorbs the lowest amount of heat energy? Metal Specific Heat Copper 0) 385 J/(g ∙ °C) Magnesium 1) 02 J/(g ∙ °C) Mercury 0) 138 J/(g ∙ °C) Silver 0) 237 J/(g ∙ °C) Lead 0) 129 J/(g ∙ °C)

Correct AnswerverifiedShow Answer

Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H2(g) + O2(g) → H2O(l) ; ΔH = -285.8 kJ

Correct AnswerverifiedShow Answer

The reaction of iron with hydrochloric acid is represented by the following thermochemical equation. Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g) ; ΔH° = -87.9 kJ How much heat is liberated at constant pressure if 0.154 g of iron reacts with 25.7 mL of 0.358 M HCl?

Correct AnswerverifiedShow Answer

The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid potassium bromate,KBrO₃?

Correct Answer
verified

What is the standard enthalpy change for the combustion of gaseous propylene,C₃H₆? C₃H₆(g) + O₂(g) → 3CO₂(g) + 3H₂O(l) Substance ΔH°_f (kJ/mol) C₃H₆(g) +20) 4 CO₂(g) -393.5 H₂O(l) -285.8

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

At constant pressure,the sign of q for the process CO₂(s) → CO₂(g) is expected to be

Correct Answer
verified

Correct Answer
verified

From the following information,determine the enthalpy of formation of C₂H₄(g) . C₂H₄(g) → C(s) + H₂(g) ; ΔH = -26.2 kJ

Correct Answer
verified

How much heat is evolved upon the complete oxidation of 6 g of aluminum at 25°C and 1 atm pressure? ( for Al₂O₃ is -1676 kJ/mol.) 4Al(s) + 3O₂(g) → 2Al₂O₃(s)

Correct Answer
verified

Given: 4AlCl₃(s) + 3O₂(g) → 2Al₂O₃(s) + 6Cl₂(g) ; ΔH = -529.0 kJ Determine ΔH for the following thermochemical equation. Cl₂(g) + Al₂O₃(s) → AlCl₃(s) +O₂(g)

Correct Answer
verified

Consider the following changes at constant temperature and pressure: H₂O(s) → H₂O(l) ; ΔH₁ H₂O(l) → H₂O(g) ; ΔH₂ H₂O(g) → H₂O(s) ; ΔH₃ Using Hess's law,the sum ΔH₁ + ΔH₂ + ΔH₃ is

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts with 29.0 L of carbon dioxide gas,measured at 1.00 atm pressure and 25.0°C? (R = 0.0821 L • atm/(K • mol) ) CaO(s) + CO₂(g) → CaCO₃(s) ; ΔH° = -178.3 kJ

Correct Answer
verified

The balanced equation representing the standard enthalpy of formation reaction for NH₃(g) is

Correct Answer
verified

What is ΔH° for the following reaction? 2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(l) Substance ΔH°_f (kJ/mol) C₂H₂(g) +226.7 CO₂(g) -393.5 H₂O(l) -285.8

Correct Answer
verified

Given the thermochemical equation 2Al(s) + O₂(g) → Al₂O₃(s) ; ΔH = -1676 kJ Find ΔH for the following reaction. 2Al₂O₃(s) → 4Al(s) + 3O₂(g)

Correct Answer
verified

The enthalpy change at 1 atm of which reaction corresponds to the standard enthalpy of formation of solid calcium nitrate,Ca(NO₃) ₂?

Correct Answer
verified

Correct Answer
verified

Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H₂(g) + O₂(g) → H₂O(l) ; ΔH = -285.8 kJ

Correct Answer
verified

The reaction of iron with hydrochloric acid is represented by the following thermochemical equation. Fe(s) + 2HCl(aq) → FeCl₂(aq) + H₂(g) ; ΔH° = -87.9 kJ How much heat is liberated at constant pressure if 0.154 g of iron reacts with 25.7 mL of 0.358 M HCl?

Correct Answer
verified